Calculate the pH of each of the following strong acid solutions. (a) 0.000726 M HClO4 pH =  (b) 0.633 g of HBrO4 in 20.0 L of solution pH =  (c) 78.0 mL of 2.30 M HClO4 diluted to 4.70 L pH =  (d) a mixture formed by adding 46.0 mL of 0.00140 M HClO4 to 49.0 mL of 0.00732 M HBrO4 pH =

Calculate the pH of the following solutions.   Ka for HClO is 2.5*10-9   a)A solution made by dissolving 4.50 g hypochlorous acid (HClO) into 1.50 L of solution.               b)A solution made by dissolving 7.40 g of potassium hypochlorite (KClO) into 1.50 L of solution.               c)A buffer is prepared by adding 4.50 grams of hypochlorous acid (HClO, Ka=2.5*10-9) and 7.40 grams of potassium hypochlorite (KClO) to a make a 1.50 L solution.

What volume of 0.1650 M NaOH is required to titrate 17.00 mL of 0.1250 M HCl?

What is the pH of a solution in which 43 mL of 0.33 M NaOH is added to 13 mL of 0.170 M HCl?

Determine the pH of (a) a 0.25 M NH3 solution.  (b) a solution that is 0.25 M NH3 and 0.40 M NH4Cl.  Kb for NH3 is 1.8 ×10−5

What volume of .155 M of NaOH is required to titrate 18.5 ml of .12 M of HCl?

A 0.251 g sample of impure NaOH requires 17.6 mL of 0.2903 M HCl for neutralization. What is the percent of NaOH in the sample, by weight?

If 15.0 mL of glacial acetic acid (pure HC2H3O2) is diluted to 1.70 L with water, what is the pH of the resulting solution? The density of glacial acetic acid is 1.05 g/mLpH=?

If 250.0 mL of HNO3 are reacted with 34.8 mL of 0.721 M Ba(OH)2, to reach the equivalence point, what is the pH of the original HNO3 solution?

What is the pH fo the following solution? 0.253 M Ba(OH)2