Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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What is the pH at the equivalence point if it requires 28.50 mL of 0.1208 M KOH to completely titrate 25.00 mL of a solution of propanoic acid, HC3H5O2?
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- A student titrates 20.00 mL of 0.300 M HCN (Ka of HCN = 4.9x10^-10) with 0.200 M NaOH. What is the pH after he adds 15.00 mL 0.200 M NaOH to the acid?arrow_forwardThe pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of carbonic acid (H2CO3) to that of the bicarbonate ion (HCO3−). (Ka1 of carbonic acid is 4.2 × 10−7.)arrow_forwardAn analytical chemist is titrating 238.1 mL of a 0.5500M solution of propionic acid (HC₂H₂CO₂) with a 0.8000M solution of KOH. The pK of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 119.8 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = X S ?arrow_forward
- An analytical chemist is titrating 144.6 mL of a 0.6600 M solution of benzoic acid (HC H,CO,) with a 0.8400 M solution of KOH. The p K, of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 54.06 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pHarrow_forwardconsider the titration of 50.0 mL of 0.10 M acetic acid with NaOH. drag and drop each amount of NaOH added (to the acetic acid) Into the appropriate resulting pH. In other words, determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solutions be acidic, basic, or neutral? Consider the stration of 50.0 ml of 0.10 M acetic acid (HC₂H₂O₂. K, -18 x 10) with NaOH. Drag and drop each amount of NaOH added to the acetic acid) into the appropriate resulting pH. In other words determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solution be acidic, basic, or neutra? Acidic Neutral Basic Drag and drop your selection from the following list to complete the answer 25.0 mL (total) of 0.10 M NaOH has been added (the halfway point) 50.0 mL. (total) of 0.10 M NaOH has been added (the equivalence point) 10.0 mL (total) of 0.10 M NaOH has been added 60.0 mL (total) of 0.10 M NaOll has been added No NaOH has been…arrow_forwardHow many grams of dry NH4Cl nned to be added to 2.50 L of a 0.200 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.69? Kb for ammonia is 1.8 x 10^-5.arrow_forward
- A student sets up a titration with 100 mL of 0.50 M HC2H3O2 and begins adding 0.25 M NaOH. What is the pH after 100 mL of NaOH have been added?arrow_forwardAn analytical chemist is titrating 149.7 mL of a 0.5500M solution of benzoic acid (HC H CO,) with a 0.8000 M solution of NaOH. The p K of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 16.29 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. do pH = Check Explanation 2021 McGraw-Hil Education. All Rights Reserved. Terms of Use Privacy Accessibility V I 11:55 acer &arrow_forwardIf 100.0 mL of 0.250 M HBr is titrated with 0.150 M KOH answer the following questions. What is the pH of the solution before the titration begins? How many milliliters of NaOH must be added to reach the equivalence point? HBr (aq) + KOH (aq) KBr (aq) + H2O (l) What is the pH of the solution at the equivalence point? What is the pH of the solution when 30.0 mL of KOH has been added? What is the pH of the solution when 180.0 mL of KOH has been added?arrow_forward
- In a titration of 68.0 mL of a 0.750 M solution of a triprotic acid H₃C₆H₅O₇ (citric acid) with 0.500 M NaOH, how many mL of base are required to reach the third equivalence point?arrow_forwardA buffer is prepared from 60.0 mL of 0.100 M formic acid(HCOOH) and 40.0 mL of 0.100 M formate (HCOO --). What is thepH of the buffer solution ? K a of formic acid is 1.78 x 10 4arrow_forwardAssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 3.00 ✕ 102 mL of solution and then titrate the solution with 0.148 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2- M H3O+ M OH-arrow_forward
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