How many grams of 3.85% (w/w) solution of KOH in water is needed to neutralize completely the acid in 13.8 mL of 0.335 M H2SO4?
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An acid solution is 0.100M in HCl and 0.210 M in H2SO4. What volume of a 0.160 M KOH solution would have to be added to 550.0 mL of the acidic solution to neutralize completely all of the acid?
(a) How many milliliters of 0.165 M HCl are needed to neutralize completely 35.0 mL of 0.101 M Ba(OH)2 solution? ml (b) How many milliliters of 3.50 M H2SO4 are needed to neutralize 25.0 g of NaOH? mL (c) If 54.8 mL of BaCl2 solution is needed to precipitate all the sulfate in a 544 mg sample of Na2SO4 (forming BaSO4), what is the molarity of the solution? M (d) If 47.5 mL of 0.250 M HCl solution is needed to neutralize a solution of Ca(OH)2, how many grams of Ca(OH)2 must be in the solution? g
You have 50 mL of 3.0 M H2SO4. How many mL of a 2.0 M solution of KOH is needed to exactly neutralize the acid?
I know the answer is 150 mL, but I need to know HOW to work this problem.