2. Next your boss hands you a solution of sulfuric acid and asks you to titrate

Question

2. Next your boss hands you a solution of sulfuric acid and asks you to titrate it with your NaOH solution. It requires 43.88mL of your standardized NaOH solution to titrate 22.54mL of the sulfuric acid solution. Write a chemical equation for the neutralization reaction and then, calculate the molarity of the sulfuric acid solution. 3.A student mixes 25.00 mL of 0.1000 M nitric acid with 40.00 mL of 0.500M potassium hydroxide solution. What substances will be present in the final solution , and what will their molarities be? 4. A Student dispenses of 25.66mL of 0.1034M HCl into a 250mL Erlenmeyer flask, adds 4 drops of phenolphthalein and then adds 33.05mL of 0.1007 M NaOH solution. What color is the solution? Why? phenolphthalein and solution? Why?

Explanation / Answer

Exp 8. Acid-Base titration

The chemicl equation is

2NaOH + H2SO4 gives Na2SO4 +2H2O

now 1000 ml of H2SO4 solution contains 98g of H2SO4

then, 22.54ml will be 98/1000 x 22.54 = 2.20M of H2SO4.

4. The color of the solution will be pink as it is basic in nature, after all the acid is completely neutralised by NaOH, the additional NaOH will remain in the solution. Since, the strength of both the solution is same, so, equal volume of base is required to neutralise the acidic solution.

3. The solution will contain KNO3 and H2O after titration of KOH with HNO3. The strength of KNO3 is 0.758 M.

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