To have a buffer with a pH of 2.50, what volume of 0.150 M NaOH must be added to 100. mL of 0.230 M H3PO4?

An important component of blood is the buffer combination of dihydrogen phosphate ion and the hydrogen phosphate ion. Consider blood with a pH of 7.44. a What is the ratio of [H2PO4] to [HPO42]? b What does the pH become if 25% of the hydrogen phosphate ions are converted to dihydrogen phosphate ion? c What does the pH become if 15% of the dihydrogen phosphate ions are converted to hydrogen phosphate ions?

When 35.0 mL of 0.200 M perchloric acid and 35.0 mL of 0.200 M potassium hypochlorite are combined, the pH of the resulting solution will be : ..... fill in the blank 1A. Less than 7B. Equal to 7C. Greater than 7

What is the minimum concentration of ammonia that should dissolve AgBr to produce a 0.01 M Ag(NH3)2^+ solution?

Using the square-bracket notation, express the concentrations of ions in a solution that is 0.750 M in aluminum sulfate [Al2(SO4)3].

Consider Al(OH)3(s) + 3H+(aq) ↔ Al 3+(aq) + 3 H2O(l)a. Calculate K for this reaction. b. Calculate the molar solubility of Al(OH)3 in acid at pH 4.0.

Hydrocholic acid (13.5 mL of 0.235 M) is added to 431.0 mL of 0.0790 M Ba(OH)2 solution. what is the concentration of the excess H+ or OH- ions left in this solution? assume that the volumes are additive.

What are the concentrations of Ag+, CN–, and Ag(CN)2 − in a saturated solution of AgCN?

What is the pH (aq., 25 oC) above which a solution of iron(III) hydroxide will precipitate? Ksp = 2.60 x 10–39.