
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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How many ml of 0.2 M HCl needs to be added to 100.0 ml of 0.2 M Sodium acetate (kb for acetate is 5.6x10-10 to achieve a pH of 4.5?
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- A solution that is made by mixing 50.0 mL of 0.15 M acetic acid and 50.0 mL of 0.20 M sodium acetate. The Ka of acetic acid is 1.8×10-5. What is the pH?arrow_forwardCalculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 100.0 mL of 0.20 M NH3. The Kb for NH3 is 1.8x10-5arrow_forward2. In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question Which is 0.1186arrow_forward
- A solution that is made by mixing 50.0 mL of 0.15 M acetic acid and 50.0 mL of 0.20 M sodium acetate. The Ka of acetic acid is 1.8×10-5. What is the pH?arrow_forwardWhat is the pH of a buffer solution that is 0.13 M methylamine and 0.21 M methylammonium chloride? (Assume the value of Kw is 1.0 10-14.)arrow_forwardHow do I complete problem 1 in a step by step?arrow_forward
- Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸. Determine the moles of the ractant and product after the reaction of the acid and base. (Similar to ICE format but is instead Before (mol), Change (mol), and After (mol) Determine the ICE table for HClO (aq) + H2O - H3O+ + ClO- (aq) Fill in Ka= ? = 2.9 * 10-8 Calculate pHarrow_forwardA 0.2649-g sample of a monoprotic acid neutralizes 53.8 mL of 0.07193 M KOH solution. Calculate the molar mass of the acid. 4.0 | g/molarrow_forwardYou need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. If you start with 0.71 M NH4Cl solution, what concentration of NH3 l will you need to also start with? (Kb for NH3 is 1.8x10-5)arrow_forward
- Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 100.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 × 10-6. ( PREV 1 Based on the result of the acid-base reaction, determine the pH of the solution. pH RESET 6.21 7.79 11.3 2.70 1.85 1.70 3.91 10.1 12.3 3.70 17.7arrow_forwardWe have 500.0 mL of a buffer solution which is 0.651 M in NH3 and 0.354 M in NH4Cl. 500.0 mL of a 0.224 M HCl solution are added. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the final pH of this solution?arrow_forward4. Consider a buffer made by adding 0.050 mol NaC2H302 and 0.040 mol HC2H3O2 to a liter of water. a) What is the pH of this buffer? b) What is the pH after addition of 0.010 mol NaOH? c) What is the pH after addition of 0.010 mol HCI to the original buffer solution?arrow_forward
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