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# 3 acid base titrations solved and explained

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How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point:

-- 45.0 mL of 0.0950 M NaOH
-- 22.5 mL of 0.118 M NH3
-- 125.0 mL of solution that contains 1.35g of NaOH per liter.

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#### Solution Preview

0.105M HCl means 0.105 moles of hydrochloric acid per liter of solution

Other useful numbers: molar mass of HCl = 36.46 g/mol
molar mass of NaOH = 39.9971 g/mol
molar mass of NH3 = 17.0306 (though it exists in solution as NH4OH, which has a mol. mass of 35.046)

Other useful facts: HCl is monoprotic, meaning it is an acid that donates only a single proton
NaOH and NH3 are ...

#### Solution Summary

The question asks for how much of a certain concentration of acid is required to titrate to equivalence 3 different amounts of 3 different bases. The solution and full explanation are given.

\$2.19

## Acid/Base Chemistry Problems

1. Solve the following problem related to the solubility of equilibria of some metal hydroxides in aqueous solution.

a) The solubility of Cu(OH)2 (solid)is 1.72x10^-6 gram per 100 ml of solution at 25 degrees C.
i. Write the balanced chemical equation for the dissociation of Cu(OH)2 (solid) in aqueous solution.
ii. Calculate the solubility (in moles/liter) if Cu(OH) 2 at 25 degrees C.
iii. Calculate the value of the solubility-product constant Ksp for Cu(OH)2 at 25 degrees C.
b) The value of the solubility product constant, Ksp, for Zn(OH) 2 is 7.7x10^-17 at 25 degrees C.
i. Calculate the solubility of Zn(OH)2 at 25 degrees C in a solution with a pH of 9.35
ii. At 25 degrees C, 50 mL of .1 molar Zn(NO3) 2 is mixed with 50mL of a .3 molar NaOH. Calculate the molar concentration of Zn2+ (aq) in the resulting solution once equilibrium has been established. Assume the volume are additive

2. A 30mL sample of a weak monoprotic acid was titrated with a standardized solution of NaOH. A pH meter was used to measure the pH after each increment of NaOH was added, and the curve attached was constructed

a) Explain how this curve could be useful determining the molarity of the acid
b) Explain how this curve could be used to determine the dissociation constant, K of the weak monoprotic acid.
c) If you were to repeat the titration using an indicator in the acid to signal the endpoint, which of the following indicators should you select? Why?
Methyl Red Ka= 1x10^-5
Cresol Red Ka= 1x10^-8
Alizarin yellow Ka= 1x10^-11

d) Sketch the titration curve that would result if the monoprotic acid were replaced by a strong monoprotic acid, such as HCL of the same molarity. Identify differences between this titration curve and the curve shown attached.

3. A buffer solution contains .4 mole of formic acid HCOOH, and .6 mol of sodium formate, HCOONa, in 1L of solution. The ionization constant, Ka, of formic acid is 1.8x10^-4

a) Calculate the pH of the solution
b) If 100mL of this buffer solution is diluted to a volume of 1L with pure water, the pH does not change. Discuss why the pH remains constant on dilution.
c) A 5.00mL sample of 1.00 molar HCL is added to 100mL of the original buffer solution. Calculate the [H3O-] of the resulting solution
d) An 800mL sample of 2 molar formic acid is mixed with 200mL of 4.8 molar NaOH. Calculate the [H3O-] of the resulting solution.

4. H3PO2, H3PO3, and H3PO4 are monoprotic, diprotic, and triprotic acids, respectively, and they are about equal weak acids.

HClO2, HClO3, and HClO4, are all monoprotic acids, but HClO2 is a weaker acid than HClO3, which a weaker acid than HClO4. Account for:

A) The fact that the molecules of the three phosphorus acids can provide different numbers of protons.

B) The fact that the three chlorine acids differ in strength.

Please see the attachments.

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