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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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The pH of a 0.10 M solution of an unknown chloride salt with the generic form of (metal ion)Cl is determined to be 4.62. Determine the cation’s Ka value.
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- An analytical chemist is titrating 191.3 mL of a 0.2000 M solution of propylamine (C,H,NH,) with a 0.1100 M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 416.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.arrow_forwardAn analytical chemist is titrating 239.5 mL of a 1.000 M solution of propionic acid (HC,H,CO, with a 0.2500 M solution of NaOH. The pK, of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 768.2 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places.arrow_forwardA buffer solution is made that is 0.485 M in HClO and 0.485 M in KClO. If Ka for HClO is 3.50x10^-8, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.129 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)arrow_forward
- 1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?arrow_forwardA 34.8 mL aliquot of weak acid that has a concentration of 0.752 M will be titrated with 0.853 M NaOH. Calculate the pH of of the solution upon the addition of 0 mL of HCl. The Ka of the acid is 7.5×10-6. A 36.54 mL aliquot of weak acid that has a concentration of 0.255 M will be titrated with 0.981 M NaOH. Calculate the pH of of the solution upon the addition of 40.11 mL of NaOH. The Kb of the base is 7.9 × 10-7.arrow_forwardA 0.381-M aqueous solution of NH3 (ammonia) has a pH of 11.4. Calculate the pH of a buffer solution that is 0.381 M in NH3 and 0.480 M in NH4+.pH =arrow_forward
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