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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Please help in solving e-f of question. Thanks
can someone explain what I did wrong. the correct answer is circled for number one, but I got 2.19 as the poh, not the pH
A 16.8 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 5.66 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:
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_forward1. What is the pH of the solution that results from adding 30.0 mL of 0.100 M NaOH to 45.0 mL of 0.100 M acetic acid? 2.87 5.05 7.00arrow_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_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_forwardYou 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_forward
- Malic 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_forwardThe 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?arrow_forwardSolve it correctly and in clear handwriting I'll upvote your answerarrow_forward
- Donarrow_forwardA 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_forwardThe next questions are related to the titration of 25 mL of a 0.0950 M acetic acid solution with 0.900 M KOH. What is the initial pH of the analyte solution?arrow_forward
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