an the following acid-conjugate base pairs be used as a buffer? Check the box corresponding to your answer. a. Ammonia and ammonium chloride ☐ Yes ☐ No b. Acetic acid and potassium acetate ☐ Yes ☐ No c. Nitric acid and sodium nitrate ☐ Yes ☐ No d. Phosphoric acid and monopotassium phosphate ☐ Yes ☐ No e. Chlorous acid and tris ☐ Yes ☐ No

A titration of an acid and base to the equivalence point results in an acidic solution. It is likely this titration involves a strong acid and a weak base. a weak acid and a strong base. a strong acid and a strong base. a weak acid and a weak base (where Ka = Kb).

Which of the following would destroy a buffer containing 0.134 moles of weak acid HA and 0.268 moles of conjugate base A -?     0.134 mol of HCl     0.186 mol of HCl     0.0670 mol of NaOH     0.0447 mol of NaOH     0.268 mol of HCl

10 What is the pH value ofo.00150 M barium hydroxide, Ba(OH): solution? A 11.48 B 11.18 2.82 D 2.52 11 During a titration between hydrogen chloride, HCl and compound X, a neutral salt solution is formed at equivalence point. What is X? A Weak base B Strong base Strong acid D. Weak acid 12 Which of the following indicators is suitable for the titration berween methylamine, CH.NH, and hydrogen chloride, HCI? Phenolphthalein Methyl red A B Alizarin yellow R D. Phenol red A voltaic cell with inert electrodes has potassium sulphate, K;SO, as its salt bridge 13 solution. Which of the following statements are correct about the salt bridge? so,- ions are oxidized at anode Salt bridge incompletes the voltaic cell circuit Migration of K' ions are to cathode compartment II II IV Salt bridge allows ions to flow through both anode and cathode compartments I and II B Il and III A III and IV D land IV Which of the following statements are not correct regarding standard hydrogen electrode, SHE? 14…

How many grams of dry NH4Cl need to be added to 2.50 L of a 0.300 M solution of ammonia, NH3 , to prepare a buffer solution that has a pH of 8.74? Kb for ammonia is 1.8×10−5 . (Please type answer no write by hend)

A 10.0 mL solution of 0.690 M NH3 is titrated with a 0.230 M HCl solution. Calculate the pH after the following additions of the HCI solution: 0.00 mL, 10.0 mL, 30.0 mL, and 40.0 mL. Round your answer to 3 decimal places.

esti alist titrates 20.0 ml of 0.20 M HBIO with 0.10 M NaOH. Galculate the pH: 1. Before the titration. 2. When the concentration of HBro equal to the concentration of Bro. 3. When number of moles of HBrO are equal to number of moles of bane added Given an acid dissociation constant, K of HBrO=23 x 10.

Calculating the pH at equivalence of a titration solution A chemist titrates 170.0 mL of a 0.0884M pyridine (CHN) solution with 0.1089 M HNO3 solution at 25 °C. Calculate the pH at equivalence. The pK of pyridine is 8.77. b Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO3 added. pH = A பா

100. mL of 0.200 M HC1 is titrated with 0.250 M NaOH.

You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20)  and 0.180 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid:                  mL sodium benzoate:           mL