A titration is performed to determine the amount of sulfuric acid, H2SO4, in a 4.30 mL sample. About 50 mL of water is added to the sample, and then it is titrated with 44.42 mL of a standard 0.4372 molar NaOH solution. What is the molar concentration of sulfuric acid in the original sample?

Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as KHP.What volume of a 0.370 M barium hydroxide solution is needed to exactly neutralize 4.24 grams of KHP ?

An aqueous solution of potassium hydroxide is standardized by titration with a 0.178 M solution of hydroiodic acid. If 25.8 mL of base are required to neutralize 22.9 mL of the acid, what is the molarity of the potassium hydroxide solution? M potassium hydroxide

Consider the following reaction H2S (g) + FeS(s) + CO2(g) →FeS2(s) + HCO2H(aq) If 2.00 g of each reactant is each dissolved in 250.0 mL of water and all the solutions are mixed together. The final volume was measured to be 750.0 mL.  a)How many grams of CO2 left unreacted?  b) What is the concentration of HCO2H in this solution?

An aqueous solution of calcium hydroxide is standardized by titration with a 0.111 M solution of hydroiodic acid. If 11.1 mL of base are required to neutralize 16.7 mL of the acid, what is the molarity of the calcium hydroxide solution? M calcium hydroxide

In the laboratory, a student dilutes 25.3 mL of a 8.46 M hydrobromic acid solution to a total volume of 100.0 mL. What is the concentration of the diluted solution?

A sample of solid Mg(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Mg(OH)2 as it could hold. A 450-mL sample of this solution was withdrawn and titrated with 0.00357 M HClO4. It required 58.3 mL of the acid solution for neutralization.What is the solubility of Mg(OH)2 in water, at the experimental temperature, in grams of Mg(OH)2 per liter of solution?

In the neutralization of aqueous acetic acid with aqueous calcium hydroxide, 55.7 mL of 0.100 M Ca(OH)2 was required to react with 15.0 mL of CH3COOH.  What was the molarity of the acetic acid solution?

An aqueous solution of sodium hydroxide is standardized by titration with a 0.119 M solution of hydroiodic acid. If 26.4 mL of base are required to neutralize 15.5 mL of the acid, what is the molarity of the sodium hydroxide solution? M sodium hydroxide

A 10.00 ml sample of a solution of acetic acid in water was titrated to the endpoint by the addition of 15.89 ml of 0.2432 M NaOH. Calculate the volume of this NaOH solution that would be required to titrate 50.00 ml of vinegar. Vinegar is 5.00% (by mass) acetic acid. Assume that the density of the vinegar solution is the same as that of water (1.00 g/ml).