2. A student titrates 30.50 mL of a 4.50 g/L monoprotic acid (HA) with 25.00 mL of 0.10 MNaOH solution.a. Determine the concentration of the monoprotic acid (the ratio of the acid to base is 1:1).Concentration (2) =4.5030.50mLb. Determine the molar mass of the acid.= 147.542M=4-50= 1800.00253. Determine the K, for a monoprotic weak acid with a pH of 3.5 at half the equivalence point.Ka = 10-3.54. What color will the solution turn indicating that the equivalence point has been reached?

Since you have posted more than one question, we will provide the solution only for the first…

2. A student titrates 30.50 mL of a 4.50 g/L monoprotic acid (HA) with 25.00 mL of 0.10 M NaOH solution. a. Determine the concentration of the monoprotic acid (the ratio of the acid to base is 1:1). Concentration (2) = 4.50 = 30.50mL b. Determine the molar mass of the acid. 4.50 147.542

2. A student titrates 30.50 mL of a 4.50 g/L monoprotic acid (HA) with 25.00 mL of 0.10 M NaOH solution. a. Determine the concentration of the monoprotic acid (the ratio of the acid to base is 1:1). Concentration (2) = 4.50 = 30.50mL b. Determine the molar mass of the acid. 4.50 147.542

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 75QAP: A student is given 0.930 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric...

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Question

2. A student titrates 30.50 mL of a 4.50 g/L monoprotic acid (HA) with 25.00 mL of 0.10 M
NaOH solution.
a. Determine the concentration of the monoprotic acid (the ratio of the acid to base is 1:1).
Concentration (2) =
4.50
30.50mL
b. Determine the molar mass of the acid.
= 147.542
M=4-50
= 180
0.0025
3. Determine the K, for a monoprotic weak acid with a pH of 3.5 at half the equivalence point.
Ka = 10-3.5
4. What color will the solution turn indicating that the equivalence point has been reached?

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