A student prepared a Kool-Aid solution from 1.3151 g of Kool-Aid in a 100mL volumetric flask. In an experiment a student used 20.15 mL of 0.0200 M NaOH to titrate a 10.00 mL aliquot of this Kool-Aid solution. To calculate the mass % of citric acid in the aliquot we use:

A student prepared a standard copper solution by combining 6.37 mL of stock 0.261 mol/L copper(II) sulfate solution with 7.02 mL of water. What is the molar concentration of Cu2+ in this solution?

The normality of an aqueous solution of hydrobromic acid is determined by titration with a 0.151 N sodium hydroxide solution. If 32.8 mL of sodium hydroxide are required to neutralize 16.7 mL of the acid, what is the normality of the hydrobromic acid solution? N

A student titrated a 50.00 mL sample of 1.00 M sodium hydroxide solution NaOH with 30.00 mL sulphuric acid solution, H2SO4. Determine the molarity (M) of the sulphuric solution

A 0.15 M solution of HCl is used to titrate 30.0 mL of a Ca(OH)2 solution of unknown concentration. If 140.0 mL of HCl is required, what is the normality of the Ca(OH)2 solution? What is the molarity?

If 23.9 g of CH₃OH (MM = 32.04 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of CH₃OH in the resulting solution?

Consider the reaction of acetic acid (HC2H3O2) in vinegar with NaOH solution If 12.00 mL of vinegar requires 19.85 mL of 0.4500 M NaOH to reach the equivalence point. What is the molarity of the vinegar solution? (Hint, write the balanced chemical reaction.) Also, what is the mass% of acetic acid in vinegar if the density of vinegar is 1.00 g/mL?

What is the percent-by-mass concentration of acetic acid (CH3COOH) in a vinegar solution that contains 65.20 g acetic acid in a 1.000−L solution? The density of this solution is 1.005 g/mL.

In titrating a H2SO4 solution, it was found that 23.66 mL of 0.2137 M NaOH would neutralize 22.04 mL of the acid.  Find the molarity of the acid solution. (Note that this is not 1:1)               unit:

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).