
Biochemistry
9th Edition
ISBN: 9781319114671
Author: Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher: W. H. Freeman
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How would you dilute 0.1 M boric acid in 1:10 ratioto 0.01M?
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- Calculate acetic acid when it requires 44.82mL of a 0.145M NaOH solution to titrate 34.95 mL of our unknown acetic acidarrow_forwardHow do you make a stock solution of 1000 ppm using a solution which Has a density of 0.842 g/mL?arrow_forwardA 100.0 mL sample of 0.200 M aqueous hydrochloric acid is added to 100.0 ml of 0.200 M aqueous ammonia in a calorimeter whose heat capacity (excluding any water) is 480.0 J/K. The following reaction occurs when the two solutions are mixed. HCl(aq)+NH,(aq)—NH_Cl(aq) The temperature increase is 2.34 °C. Calculate AH per mole of HCI and NH, reacted. Select one: о a. -1.96 KJ/mol b. 154 KJ/mol O c. 485 KJ/mol d. 1.96 KJ/mol Jm e. -154 J/molarrow_forward
- What kind of buffer would you make with a optimal activity at ph 4.30?arrow_forwardHow many grams of CuSO4 would you use to make 1 L of an 8 g/L CuSO4 solution?arrow_forwardCalculate the pH of a buffer that contains 0.75 M acetic acid and 0.35 M acetate ion in 1 L solution. What will the pH of the buffer be upon the addition of 100.0 mL of 1.0 M NaOH? (Ka of acetic acid is 1.75 x 10-5 M)arrow_forward
- 9. (1 pt) What is the [H+] and [OH-] for the following strong acid and strong base solutions: A) 0.35 M NaOH B) 1.2 M HCI C) 0.0800 M H2SO4arrow_forwardEstimate the pH of a solution prepared by dissolving 1.0 × 10-10 mole of a strong acid in a liter of water at 25°C.arrow_forwardConsider the following acids and their ionization constant, determine which conjugate base is HCOOH Ka = 1.7 x 10-4 (b) HCN Ka = 4.9 x 10-10arrow_forward
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