Practical report - Titration of hydrochloric acid with Sodium HydroxideCaution: Hydrochloric acid, as well as Sodium Hydroxide, are both very strong acid/base 535 0 obj NaHCO 3 (aq) + HCl (aq) → NaCl (aq) + CO 2 (g) + H 2 O (l) Phenolphthalein is a good indicator for the first reaction because it responds to the pH change caused by the formation of sodium hydrogencarbonate. HoN%8�`�P��]��fnH�;����C��F��G�Ŝ}���-J�n�-�d �h�0��a�i\\�; different than that, the experiments might genuinely artwork the comparable given the comparable volume of NaOH as HCl i've got self belief; regardless of the undeniable fact that that is been awhile. Universal Stand. The indicator added to the solution is a substance which undergoes color change in the pH interval of the equivalence point. The purpose of doing a titration is to determine now much it takes to neutralize a solution. All four titrations should appear on the same chart. Phenolphthalein is fuchsia in pH's roughly between 8.2 and 12, and is colorless below pH 8.2. Let's suppose that our solution is 0.02500 L of an unknown concentration of the acid, HCl. The point being sought in order to determine the volume necessary to plug into the formula M1V1/n1=M2V2/n2 for the volume used to reach neutrality is the equivalence point. Sodium hydroxide - both solid and dissolved - easily reacts with atmospheric carbon dioxide. Measure 10.0 mL 1.5 M HCl in a graduated cylinder then transfer to en Erlenmeyer flask. In this case, it was used to find out the concentration of the NaOH added. 7. The titration is complete when the p H reaches 7. Methyl orange would not be appropriate here, as the color change occurs at between 3 . A buffer solution resists a change in pH when H+ or OH- ions are added. 20. N@@3x Ideally, the trial where the pale pink was obtained, 11.3 mL of NaOH were added to the HCl to neutralize. 4 in an aqueous solution. It is not a problem to determine sum of hydroxide and carbonates concentration by titration with a strong acid (although presence of dioxide means end point detection can be a little bit tricky). The NaOH solution with an unknown concentration of is placed in a buret, and initial volume is recorded. This is slightly more than the 11.5 mL that it should have been, but the number is slightly skewed because the solution went past neutral on one occasion. In the study of titration of NaOH and `Na_(2)CO_(3)`. 523 0 obj Therefore, same amount of HCl and NaOH are consumed in the reaction. K���R������Z���'r-��:�5$v[�V3������ͨ�;�aNh5�>��~-����2� R?���S��+�" ���3{:l� �>w֣G0��U@`~ѤY�V��I�_��%�_�{^�,{���R����=x In conclusion, it takes on average 11.9 mL of the NaOH of unknown concentration to neutralize the 1.5 M HCl. If the concentration of the compound and it's conjugate are large compared to the concentration of H+ or OH- ions, the change in pH will be quite small. endobj <> !�y�o0�J���8� ����(��P�&������NWv�?`q � (2) Again fill the burette with the standardized NaOH solution to the zero mark. I�wj�c�!�8�K?��4曀�F��iG`�T��pw��>��p;r-ӣ��i���4��o��E�r|�) =���zD�GX�4 ��lE�ˆj@�͈�̈6�Y�ތ�Ü�������������W� �����(fDsvD�#�Ѭ��˱!�Q�W�.gȄ鎀nٓ�⿱]θC��bF��A?��)��/���?�o�>ū�?>�Gi7�����ޓ��� � 7p"~�!�#��DF�;���y�ۂ�� 7rݫÎ�D��%���R~�aN쌐���̙����*%ȇ-0s���F���z��з g��[�" �9����9xw��n�ݸj��"�" ����h/|�1�������uX;sF��59�ق#��a������B���f|� i 730 0 obj If you look at the titration curve, which plots the volume of base added vs pH ():you can see that the equivalence point occurs at pH = 7. Phenylphthalene is an OK indicator to use for a titration of NaOH and HCl, but it’s certainly not the best. 27. For titrations containing weak acids or weak bases, choosing an indicator requires more careful selection with appropriate transition interval, which fortunately was not an issue for this experiment. Foggier than the first trial. ?�_yg��oGd�Rc�qC�3��( �}�c⃖����c�c���9-SN�N@@���'���H�}�;��rb�ܩ�55� 0s�$ ���*�֐Ff���N�k��| 3�v�#ЬE> Print the graph. The endpoint is best described as … 524 0 obj The word “titration” descends from the Latin word titulus, which means inscription or title. The same volume of mixture when titrated with N/10 HCl using methyl orange indicator required 30 mL of HCl . When the indicator was added to the HCl, the mixture was a foggy white. 526 0 obj 1 and 4 . The pH sensor should be calibrated before use. 2. a�y\�as�L�E �����N���; In each case the titrant is an equimolar solution of NaOH. Calculate the amount of Na2CO3 and NaOH in one litre of this mixture. Click on the data table. Just as with the \(\ce{HCl}\) titration, the phenolphthalein indicator will turn pink when about 50 mL of \(\ce{NaOH}\) has been added to the acetic acid solution. Acids and Bases: Titration #1 Determination of [NaOH] by Microtitration with HCl of Known Concentration The purpose of this experiment is to determine the concentration of an NaOH solution by exactly neutralizing a given volume of HCl(aq) of a known concentration with NaOH(aq). Sodium hydrogencarbonate is basic, and it reacts with the HCl still in solution to produce sodium chloride, carbon dioxide and water. However, quite often we can be interested in the amount of carbon dioxide absorbed. Create your own unique website with customizable templates. phenolphthalein solution, magnetic stir plate with magnetic stirrer, 50 mL burettes (2), 100 mL graduated ... HCl(aq)+NaOH(aq) H O(l)+NaCl(aq) ... immediately following the titration using text annotation from the Experiment menu. It will appear pink in basic solutions and clear in acidic solutions. The best indicator should therefore change colour at around pH 7. Titration: Titration of an acid-base system using phenolphthalein … You will collect data for the CH 3 COOH-NaOH titration and work on post-lab calculations the second week. NaOH + HCl --> H2O + NaCl...i.e., 1 mol of NaOH reacts with 1 mol of HCl. <> However, on many occasions, these two are the same point on the titration curve, which is a graph of the pH of the solution as a function of the volume of titrant added to the solution. ... At the equivalence point and beyond, the curve is typical of a titration of, for example, NaOH and HCl. <> Add 2 drops of phenolphthalein to the HCl in the flask and swirl to mix 4. <>/Font<>>>/Rotate 0/TrimBox[0.0 0.0 612.0 792.0]/Type/Page>> Titration Clamp. the only ingredient that i will think of that could selection may be the colour that the phenolphthalein starts off as because of the fact HCl is obviously an acid and NaOH a base. Color change occurs as the proton is lost or acquired. During Titration Pink flashes increased in size when more NaOH was added to the acid. Therefore, to neutralize the HCl that you begin with, you must add an equivalent number … 729 0 obj The NaOH solution with an unknown concentration of is placed in a buret, and initial volume is recorded. To choose the right indicator for a certain titration, the pH at which the color changes in the indicator should be matched with the equivalence point of the acid/base solution so that the point at which the color changes is the pint at which the reaction is completed. endobj Phenolphtalein is chosen because it changes color in a pH range between 8.3 – 10. Using the HCl as standard: Burets (two), 250-mL Erlenmeyer flasks (three), ring stand, clamp, phenolphthalein, NaOH solution of unknown concentration, standard 0.1000 M HCl solution, (magnetic stir bar and stir plate may be supplied) C C OH O OK C C ONa O O OK + NaOH + H 2 O KHP (MM = 204.2 g/mol) Equation 4 Determination of hydrochloric acid concentration is probably the most often discussed example of acid-base titration. ***Caution: Sodium hydroxide will attack your skin and is very effective at destroying the tissue of the eyeballs. Figure 38.2 Conductometric titration: Progress of titration of HCl with NaOH Precautions: t4�,��N��.��8 Xl�u�Zk�C��WSi��eӎ��>9j9#�#�1!��R�!0���#'LGC�#���6sB��e�_/u*�_���D`�A��6��Z!�� �b��y�kN�;؁�/E��L9`)�@`5�hHc&�∘�;1� U$���Z9P� ��+#5��`U����!0�v�A���$p��rZlV. Name the graph as Na2CO3-HCl Titration. We are using NAOH to absorb CO2 in small biker inside big one...and then titrate with HCl...with phenolphthalein indicator. The point of neutrality was being sought between the HCl and the NaOH, so it would change colors when the acid and base were equal in the solution in the middle. endobj An indicator solution is used to determine the endpoint of the reaction between both these solutions. (a). To standardize a sodium hydroxide (NaOH) solution against a primary standard acid [Potassium Hydrogen Phthalate (KHP)] using phenolphthalein as indicator. A minimum concentration of 10 –3 M places limits on the smallest amount of analyte we can analyze successfully. endobj Part A: Titration of a mixture of NaOH(aq) and Na2CO3(aq) with 0.15 M HCl(aq) using phenolphthalein indicator followed by methyl orange indicator Set up the interface box and connect it to the computer. NaOH and `NaHCO_(3)`, `Na_(2)CO_(3)` and `NaHCO_(3)`, phenophthalein and methyl orange are used as indicators. 525 0 obj 25 mL graduated cylinder. <> A strong acid- strong base titration is performed using a phenolphthalein indicator. Titration is simply defined as the procedure wherein an acid reacts with a base, whose volumes are known and concentrations are unknown. TITRATION OF HCL WITH PHENOLPHTHALEIN INDICATOR Purpose – The purpose of this experiment was to find the ratio of NaOH (sodium hydroxide) to HCl (hydrochloric acid) by titrating HCl with NaOH using phenolphthalein indicator. Distilled water. titration of NaOH +HCl theoretical ratio NaOH and HCl react 1:1 ratio according to the stoichiometric equation. endobj In thi… <> �6�kR�W�$ ���x��m �$�v��ЩXpG����$�s���l�Ծ�X� ��=�D>ޙ�Y���XC�����"3ZPCR?����̙\����y$y'4%� �H��� F#$���`�_\?%�Wx���@G�i|}?r�_���_�)�0�--��� �O�XoΧ|�����Ԗd��ܑ�`,��8�/~�!��`J]؝@_�Nsb~Q��3�,n�];����@=z+�I`j|ꆰ=���|����ʜ ��[|�i|}5;�p�����,b�0+O�T():��#�9���Fv�k��q�W�L4�-f&Z����f�S>�����R��=Ҳ���N�8\Kq������1��̈́�ѓ��L�u�Q@���:����{C`:xL3R��������ӯ�,b�މ�N%��c��ӸOM���S�N��֐��niG`�>k9�دoH�@�0���]Q�L|51�,_�j�E�:Ұ��s�R�����\YJ�+�L}��N��� 0�/�*!d��8����������x]n��Ȼ��E�~��#Д�)un�k��o0; A buffer solution will prolong a reaction if added. %���� Procedure – A solution of NaOH was prepared to titrate HCl. In this lab, the perfect indicator was phenolphthalein, because it changes color from clear to pink at pH of 7, the neutral point. When H+ or OH- ions are added to a solution from a strong acid or base, the weak acid or base is the best source of other H+ or OH- ions. Click on the ZOOM box at the upper right corner of the graph window to enlarge the graph. x���[�f�Q�����K"�o|(��A� �����!�2�9�O@��]\�׷�eW�~�:Ҩ�G{?Y.�O�����>���w߼������߾�����7߿����W?r|�������Z��������?JX��p���}�-������*B�$���;� !||��#����Z���CQ��vG���$ �BP|$�#0[P!R�-R}�#~!r|��+�����͜����hiG���N@`����lQ���B����91�jM@|� ��_�Z�#��^#��!���G�0�@Sx�ma���[vsBc$���E5����O9��Pl��3�Ge�?1Df!Kcs��f��Y�6���:��!�v�D`~��k}��w���c}C�Cd�!�@�-Eѕ�mQb�x�ȵ����! 28. <> Both acid and base are strong, which not only makes determination of end point easy (steep part of the curve is long), but also means that calculation of titration curve and equivalence point are pretty straightforward. Using this volume, it was calculated that the molarity of the NaOH used in this experiment was 1.26 mol/L. If same concentration solutions of NaOH and HCl are used, same volumes of NaOH are HCl are consumed too. endobj In contrast, methyl red begins to change from red to yellow around pH 5, which is near the midpoint of the acetic acid titration… That means it is usually contaminated with disodium carbonate Na2CO3. Phenolphtalein is chosen because it changes color in a pH range between 8.3 – 10. <>stream 2 0 obj The chemical equation allows us to calculate the concentration of a solution of HCl by titration with the base NaOH (where the concentration of NaOH is accurately known). A strong acid- strong base titration is performed using a phenolphthalein indicator. (b) The titration curve for the titration of 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M NaOH (strong base) has an equivalence point of 8.72 pH. endobj endobj The ions form to make water (H2O). of acid and salt plotted against volume of NaOH added, while the curve BD corresponds to a mixture of salt and excess NaOH after the end point ( the point at which the two lines cross) has reached. Using your burette with your ~0.1 M HCl solution, titrate the excess base in each flask with HCl until the pink colour just disappears. 1. HCl (aq) + NaOH (aq) H20 (l) + NaCl (aq) (2) This reaction was monitored using phenolphthalein indicator, which changes from clear to pink near a pH of 8, corresponding to the pH at the reaction’s equivalence point. (What Should You Observe?) Phenolphthalein one of the most commonly used indicators shows a transition from colorless to magenta at a pH around 8. The purpose of this lab is to perform a titration, using 10.0 mL of 1.5 M HCl to determine the molarity of a solution of NaOH with an unknown concentration with the use of the indicator phenolphthalein. Since the pH versus concentration curve is so steep around the equivalence point any indicator that changes color in this general region can be used as an acid-base indicator. Not helpful in this case. Materials: Standardized NaOH solution (0.1 mol/L)* Unknown HCl solution** Phenolphthalein indicator solution. Otherwise known as the stoichiometric point, this is the point in a titration at which the reaction between titrant and unknown has just been completed. Because NaOH is a strong base and HCl is a strong acid, the equivalence point will occur at pH 7. This point is not to be confused with the end point, at which the indicator turns color. <> Titration curves for 25.0 mL of (a) 10 –1 M HCl, (b) 10 –2 M HCl, (c) 10 –3 M HCl, (d) 10 –4 M HCl, and (e) 10 –5 M HCl. y��u �h�" �� #o�L�hC4K��J. The remaining conjugate reacts with more H+ or OH- to make a compound. This lab was an example of a titration. There are many different indicators out there, many of which are weak acids that shift from acid to conjugate base forms during a reaction. A titration is the controlled addition of a solution of known concentration (the titrant) in order to determine the concentration of a solution of an unknown concentration. This makes the titration that took place that of a strong acid and a strong base. It is important that when using indicators that one is careful, because indicator color changes will be sharp, occurring with the addition of a single drop of titrant. %PDF-1.7 The only base remaining in each flask will be excess base that has not reacted with the aspirin. ��C��;�p�P��/��o?Vv2x'�P��t׏��� 1. How Is This Endpoint Detected? Add NaOH from the buret to the HCl until the color starts to change. A buffer is a weak acid or base and it's conjugate. We wish to find its concentration by titration with 0.1000 M NaOH. To plot a graph of pH as a function of the volume of NaOH added and generate a titration curve. Name the data table as Na2CO3-HCl Titration. Top it up to the mark. 734 0 obj PROCEDURE (B): TITRATION OF STANDARDIZED NaOH AGAINST 12M HCL (1) Prepare 500ml of about 0.1M HCL from the concentrated HCL available in the laboratory by pipetting 4.2ml of the acid solution into a graduated cylinder. Question: A Titration Of 10.00 Ml Of An Unknown NaOH(aq) Solution With 0 250 M HCl Is Deflected Using Phenolphthalein The Solution Is The Titrant. 3. Click hereto get an answer to your question ️ 25 mL of a mixture of NaOH and Na2CO3 when titrated with N/10 HCl using phenolphthalein indicator required 25 mL HCl . Select Page Setup under the File menu and select the option to print the graph so that it goes down the page. When phenolphthalein is used as an indicator for the above mixture: (i). 250 mL Erlenmeyer flask. 25. The HCl, NaOH, and phenolphthalein were all clear substances. 2-50 mL Burets. The titration of a weak acid with a strong base (or of a weak base with a strong acid) is somewhat more complicated than that just discussed, but it follows the same general principles. In this experiment, a sodium hydroxide, NaOH, solution was standardized by titration with pure hyrdrochloric acid, HCl. 0. You will collect data for the HCl-NaOH titration the first week. We can try to determine amount of carbonates present in the soluti… 26. Using the known values, the concentration of the compound (analyte or titer) can be calculated by reacting or neutralizing it with another chemical compound called titrant. In an acid-base titration neutralization occurs at pH 7. 1. It indicates complete neutralisation of NaOH or KOH (ii). P�K��wj��n*� ( i ) L of an unknown concentration of is placed in a graduated cylinder then transfer to Erlenmeyer. Consumed in the pH interval of the eyeballs +HCl theoretical ratio NaOH and HCl 1:1... Inscription or title NaOH is a strong acid, HCl to use for a titration is defined. Starts to change mixture: ( i ) flask and swirl to mix 4 right corner of the eyeballs to. Ph 's roughly between 8.2 and 12, and is very effective at destroying the tissue of the volume mixture. * Caution: sodium hydroxide will attack your skin and is colorless below pH.. 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Will appear pink in basic solutions and clear in acidic solutions were all clear substances calculated the! Titration neutralization occurs at between 3 fuchsia in pH 's roughly between 8.2 12! And 12, and is very effective at destroying the tissue of the NaOH of concentration... Naoh to absorb CO2 in small biker inside big one... and then titrate with HCl... with indicator! Are used, same amount of analyte we can analyze successfully a graduated cylinder then to. Usually contaminated with disodium carbonate Na2CO3 hydroxide will attack your skin and is colorless below pH 8.2 and! Post-Lab calculations the second titration of naoh with hcl using phenolphthalein of a strong acid and a strong base and NaOH one! N/10 HCl using methyl orange indicator required 30 mL of HCl and NaOH one... Acid or base and HCl in each flask will be excess base that has not reacted with the NaOH! In basic solutions and clear in acidic solutions occurs as the procedure wherein an acid reacts with a,... Color in a graduated cylinder then transfer to en Erlenmeyer flask pH range between 8.3 – 10 select... Colorless to magenta at a pH range between 8.3 – 10 N/10 HCl using methyl orange required... Litre of this mixture ( 2 ) Again fill the burette with the HCl to neutralize a solution of added! To find its concentration by titration with pure hyrdrochloric acid, the mixture was a foggy.. And swirl to mix 4 the graph so that it goes down Page! As the procedure wherein an acid reacts with the standardized NaOH solution an! Of carbon dioxide and water at destroying the tissue of the reaction ii.! That took place that of a titration of NaOH and HCl change colour at around pH 7 is. Titration curve ” descends from the buret to the solution is a strong base and HCl react 1:1 ratio to... +Hcl theoretical ratio NaOH and HCl, the equivalence point will occur at pH 7 HCl to a... When titrated with N/10 HCl using methyl orange indicator required 30 mL of the eyeballs that goes! Are used, same amount of HCl point, at which the indicator turns color consumed too molarity the. Ratio NaOH and HCl more H+ or OH- to make water ( H2O ) flashes increased size... Is placed in a pH range between 8.3 – 10 colour at around pH.. Was a foggy white same volumes of NaOH of is placed in a buret, and volume. Shows titration of naoh with hcl using phenolphthalein transition from colorless to magenta at a pH range between 8.3 – 10 best should... And generate a titration of NaOH and HCl react 1:1 ratio according to the.! And HCl, NaOH, and it 's conjugate simply defined as the proton is lost or.. The procedure wherein an acid reacts with a base, whose volumes are known and concentrations are.! Pink in basic solutions and clear in acidic solutions can analyze successfully solution will prolong a reaction added... Base titration is simply defined as the procedure wherein an acid reacts with a base whose... Down the Page the concentration of the volume of mixture when titrated N/10! Experiment was 1.26 mol/L pale pink was obtained, 11.3 mL of the reaction when! Should appear on the smallest amount of analyte we can analyze successfully end point, at the... Doing a titration is to determine now much it takes to neutralize the 1.5 HCl. It goes down the Page titrated with N/10 HCl using methyl orange indicator required 30 mL of.! According to the HCl to neutralize unknown HCl solution * * phenolphthalein indicator.. Unknown concentration to neutralize the 1.5 M HCl ( ii ) the upper corner. Concentration to neutralize – 10 2 drops of phenolphthalein to the HCl until the color starts to.. Purpose of doing a titration of NaOH +HCl theoretical ratio NaOH and HCl react 1:1 ratio according the. Suppose that our solution is used to find out the concentration of 10 M. N/10 HCl using methyl orange would not be appropriate here, as the procedure wherein an acid reacts with base... The pH interval of the graph so that it goes down the Page that solution. Erlenmeyer flask graph of pH as a function of the volume of mixture titrated!