What is the pH of a solution prepared by diluting 0.040 mol HNO3(aq) to a volume of 225 mL? (Hint: calculate molarity of HNO3 first) A. -0.25 B. 0.25 C. 0.040 D. 0.75 E. 0.225

The pOH of an aqueous solution at 25°C was found to be 11.00. The pH of this solution is The hydronium ion concentration is The hydroxide ion concentration is M. M.

0.60 M HIO (aq), 0.60 M HIO₂ (aq) and 0.60 M HIO₃ (aq) are randomly placed in 3 different bottles labeled as A, B, and C. If the solution in bottle B has the highest pH and the solution in bottle A has the lowest pH. Which of the following statements is correct? (Choose one option). a. Bottle B is HIO₃ (aq). b. Bottle A is HIO₂ (aq). c. Bottle A is HIO (aq). d. Bottle B is HIO₂ (aq). e. Bottle C is HIO₂ (aq).

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0199 M solution. The pH of the resulting solution is 2.31.2.31. Calculate the p?a for the acid.

What mass of KOH is necessary to prepare 830.0 ml of a solution having a pH = 11.49? Mass = g

Determine the final pH of a 1.00 L solution where 0.45 moles HBrO(aq), 0.70 moles KBrO(aq) and 0.20 moles HBr(aq) are mixed. Express your final answer to 2 decimal places. No scientific notation. Your Answer: Your A Cu

Calculate the pH of the solution: a. 1.45MCH3NH3NO3 solution. ( = (4.4 × 10¯