6.9 g of citric acid (MM =following balanced chemical equation.192.1 g/mol) can be titrated with NaOH according to the%3DH3C,H5O7 (aq) + N2OH(aq) → H20(1) + Na H2C,H507(aq)a) Choose the correct titration curve for the titration of the neutralization of the threehydrogens of this acid with NaOH.PHPHpHTitrantTitrantATitrantBPHPHpHTitrantTitrantDTitrantPH PHpHTitrantTitrantTitrantPHpHpHTitrantTitrantTitrantpHDHpHTitrantTitrantTitrantb) What volume of 0.23 M NaOH is needed to add to titrate H¿C,H;O, to NaH,C.H,O (as indicated in the equation)

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6.9 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. %3D H3C,H5O7 (aq) + N2OH(aq) → H20(1) + Na H2C,H5O7(aq) a) Choose the correct titration curve for the titration of the neutralization of the three hydrogens of this acid with NaOH. PH PH pH Titrant A Titrant Titrant PH PH PH Titrant Titrant Titrant

6.9 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. %3D H3C,H5O7 (aq) + N2OH(aq) → H20(1) + Na H2C,H5O7(aq) a) Choose the correct titration curve for the titration of the neutralization of the three hydrogens of this acid with NaOH. PH PH pH Titrant A Titrant Titrant PH PH PH Titrant Titrant Titrant

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.102QE

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7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. H3C6H5O7 (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?
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A student performed titration to determine the concentration of citric acid with potassium permanganate solution. The net ionic equation is as follows: 5C6H8O7 + 18MnO4- + 54H+ → 30CO2 + 47H2O + 18Mn2+ The concentration of potassium permanganate soluiton is 0.266 M. The volume of lemon juice is 25.00 mL. The titration consumed 17.6 mL of potassium permanganate solution to reach the endpoint. Determine the moles of citric acid in the lemon juice sample.
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You prepare a standard NaOH solution for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC₆H₇O₆, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 17.54 mL of the NaOH to titrate (react exactly with) the ascorbic acid found in one 500.0 mg tablet. What is the percent vitamin C by mass in the tablet?
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Consider the following reactions: Reaction 1: HCIO, + KOH → KC1O, + H;O Reaction 2: HC;H;O2 + KOH → KC;H;O2+ H;O In both reactions, 15.00 mL of 0.8116 M acid is titrated with 0.4217 M KOH. A volume of 28.87 mL of KOH is required to reach the equivalence point in both reactions. a) What is the pH of the HC1O, solution before the titration has started? (No KOH has been added.) b) What is the initial pH of HC;H;O2 solution before the titration has started? K= 6.46 x 10-5 (Ok to use x is small.) c) What is the pH of Reaction 1 at the equivalence point? d) What is the pH of Reaction 2 at the equivalence point? e) What is the pH of Reaction 1 after 32.00 mL of KOH has been added? f) What is the pH of Reaction 2 after 18.00 mL of KOH has been added?

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