Question

10. Calculate the pH of a solution made by mixing 10,0 mL of 0.100 HCI and 150 ml of 0.100 M NOH. 11. Indicate each of the following aqueous solutions is acidic, basic, or neutral: KOH 12. A metal complex is Cr(HO) Bra a) Name the complex (25 pt) b) Give formulas of ligands. c) What is charge of Cr? d) Find the coordination number of the complex e) Sketch all possible geometric isomers, labeling cis/trans.

Answer 1

10.

At neutralization point

mmoles of HCl = mmoles of NaOH

Given, mmoles of HCl = 10.0× 1.00 = 10

mmoles of NaOH = 15×1.00 = 15

Hence, excess mmoles of NaOH = (15-10) = 5

NaOH is strong base, disdoviates completely

Molarity of OH^- = ( mmoles of NaOH/total volume)

= $\frac{5 \: mmoles}{ [10+15]\: (mL)}$

= 0.2 mol/L or M

Now, pOH = - log[OH^-] = - log(0.2) = 0.698

Or, pH = 14 - 0.698 = 13.302

11.

KF is salt of weak acid HF and strong base KOH, hence pH of aquous solution is greater than 7, hence acidic

KI is a salt of strong acid HI and strong base KOH, hence aquoues solution of KI will be neutral.

HI is a strong acid , aqueous solution is acidic .

KOH is strong base. Its aqueous solution will be basic.