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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:Butanoic acid is a monoprotic acid with Ka = 1.51*10-5. A 35.00
mL sample of 0.500M butanoic acid is titrated with 0.200M KOH.
Find the volume of KOH solution needed to reach the equivalence
point for the titration.
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- 30 mL of 0.1 M HCI is titrated with 0.1 M CH3NH₂ (Ka = 2.0 x 10-¹1) solution. Calculate the pH after adding 15 mL of CH3NH₂ to initial acid 12.01 5.81 1.48 3.49 9.57arrow_forwardA 25. mL sample of a weak acid solution (KA= 4.3×10−4) is titrated with 0.20 M NaOH. 20.0 mL of NaOH are needed to reach the equivalence point What is the pH halfway to the equivalence point? 3.37 5.85 4.16 4.74arrow_forwardCalculate the pH at the equivalence point for the following titration: 0.30 M HC1 versus 0.30 M methylamine (CH₂NH₂). Round your answer to 2 decimal places. Note: The K of methylammonium is 2.21 × 10-¹¹. pH =arrow_forward
- A 100.0 mL aliquot of a 0.100 M solution of benzoic acid (C6H5COOH, Ka = 1.2 x 10-4) is titrated with 0.500 M NaOH. Calculate the pH at the equivalence point for this titration.arrow_forwardConsider the titration of 50. ml of a 0.10 M benzoic acid solution (HC7H5O2 Ka = 6.5 x 10^-5 ) with 0.20 M KOH. Determine each quantity: 1. The volume of base required to reach the equivalence pointarrow_forwardConsider the titration of a 25.0mL sample of 0.195M acetic acid (CH3COOH) with 0.300M NaOH. How many mL of NaOH is required to reach the equivalence point? The Ka of acetic acid is 1.8x10-5.arrow_forward
- An analytical chemist is titrating 143.8mL of a 0.7500M solution of acetic acid HCH3CO2 with a 0.4100M solution of KOH. The pKa of acetic acid is 4.70 .Calculate the pH of the acid solution after the chemist has added 283.1mL of the KOH solution to it. Round your answer to 2 decimal places.arrow_forwardCalculate the pH for each of the cases in the titration of 25.0 mL of 0.110 M pyridine, C₁H₁N(aq) with 0.110 M HBr(aq). The Kb of pyridine is 1.7 x 10-⁹. before addition of any HBr pH = after addition of 12.5 mL of HBr after addition of 16.0 mL of HBr after addition of 25.0 mL of HBr after addition of 35.0 mL of HBr 9.31 pH = pH = pH = pH = 5.23 4.63 Incorrect 11.65 Incorrect 1.33 Incorrectarrow_forwardIn the titration of a 25.0-mL sample of 0.145 M HCOOH with 0.122 M NaOH, where K, HCOOH = 1.8x10-4 %3D the volume of NAOH added at one-half the equivalence point is about 27.4 mL O the volume of NaOH added at one-half the equivalence point is about 7.45 mL O the volume of NaOH added at one-half the equivalence point is about 12.6 mL O the volume of NaOH added at one-half the equivalence point is about 14.9 mLarrow_forward
- Calculate the pH at the given points in the titration between 100.0 mL of 0.05000 m NH3 (Kb = 1.8 x 10-5) after adding the following volumes of 0.100 m HCI: 50.00 mL HCIarrow_forward12.0 10.0 8.0 A pH 6.0 4.0 2.0 0.0 C 0 5 10 15 20 25 30 mL of 0.1 M NaOH The graph above shows the titration curves of four monoprotic acids of varying strengths. All of the acids start out at 0.1 M concentration and 25.0 mL volume. Choose all of the correct statements about these titration curves from the choices below. The titration curve labelled "D" is generated by the strongest acid in the series. In the curves shown above the stronger the acid the less NaOH required for neutralization. The stronger the acid the more important is the pKa of the Indicator used for titration. The Ka of the acid which generates curve "C" is about 103 The weaker the acid the lower the pH of the neutralization point. The acid which generates curve "D" has the highest neutralization-point pH in the series.arrow_forwardA 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of hydrofluoric acid is 3.5 × 10-4.arrow_forward
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