Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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Chapter 24, Problem 2ASA
In an
- First note the value of MH+ in the HCl solution. ____________M
- Find MOH- in the NaOH solution. (Use Eq.3.) ____________M
- Obtain MNaOH from MOH. ____________M
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The next 11 questions are related to the titration of 40.00 mL of a 0.0900 M acetic acid solution with 0.0950 M KOH. Assume that the temperature is 25 oC.
What is the pH when 23.00 mL of the KOH solution have been added?
What is the pH when 46.00 mL of the KOH solution have been added?
A 19.7 mL solution of 0.100 mol L-¹ CH3COOH is
titrated using 0.150 mol L-1 NaOH.
What is the pH of the solution after 5.11 mL of the
NaOH solution is added? Express your answer to 2
decimal places.
Remember you can find KA and/or KB values in your
textbook in chapter 15. They are also posted on
eClass.
Answer:
When 25 .00 mL of 0.1098 M HCl in 40 mL of DI water is titrated against 0.09998 M NaOH, the pH increases.
What is the volume (in mL) of NaOH required to reach the equivalence point and a pH of 7.00?
Find the pH when the volume of NaOH added is 0.05 mL less than the volume required to reach the equivalence point.
Find the pH when the volume of NaOH added is 0.025 mL less than the volume required to reach the equivalence point.
Chapter 24 Solutions
Chemical Principles in the Laboratory
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- Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?arrow_forwardEnough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Âarrow_forward1. What is the pH after 25.0 ml of 0.100 M NaOH has been added to 50.0 ml of 0.100 M HCl? 1.00 1.48 7.00 13.00arrow_forward
- Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.arrow_forwardA friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?arrow_forwardA student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.arrow_forward
- You have 0.10-mol samples of three acids identified simply as HX, HY, and HZ. For each acid, you make up 0.10 M solutions by adding sufficient water to each of the acid samples. When you measure the pH of these samples, you find that the pH of HX is greater than the pH of HY, which in turn is greater than the pH of HZ. a Which of the acids is the least ionized in its solution? b Which acid has the largest Kd?arrow_forwardMethyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?arrow_forwardMalic acid is a weak diprotic organic acid with Ka1 = 4.0 104 and Ka2 = 9.0 105. a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about one molar in malic acid. c Calculate the pH of a 0.0175 M malic acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentrationin in solutions b and c?arrow_forward
- A 25.00 mL sample of 0.1000 CH3COOH is titrated with a 0.1000 M NaOH solution. Calculate the pH after the addition of 37.33 mL of the NaOH. Be sure to use at least 4 significant figures throughout your calculations, you can only be off by 0.1 pH units. Answer: The correct answer is: 12.296arrow_forwardYou begin with 100 mL of 0,250 M HCN and add to it 0,75 M NaOH at 25°C (HCN Ka = 6,2 * 10-10) Calculate the pH after 0.0 mL of NaOH has been added. Calculate the pH after 50.0 mL of NaOH has been added. Calculate the pH after 75.0 mL of NaOH has been added. Calculate the pH at the equivalence point. Calculate the pH after 150 mL of NaOH has been added. Please be quite espisific on each steparrow_forwardIn an acid-base titration, 25.62 mL of an NaOH solution are needed to neutralize 26.23 mL of a 0.1036 M HCl solution. Use these steps to find the molarity of the NaOH. First note the value of MH+ in the HCl solution. Find MOH- in the NaOH solution. (MH+*Vacid= MOH-*Vbase ) Obtain MNaOH from MOH-arrow_forward
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