Question

Asked Oct 30, 2019

a) 0.132g of a pure carboxylic acid (R-COOH) was dissolved in 25.00mL of water and titrated with 0.120M of standardised NaOH solution.

A volume of 14.80mL was required to reach the endpoint of the titration.

Identify the carboxylic acid.

b) A 0.670g sample of barium hydroxide is dissolved and diluted to the calibration mark in a 250.0mL volumetric flask. It was found that 11.56mL of this solution was needed to neutralise 25.00mL of nitric acid solution.

Calculate the molarity of the nitric acid solution. Write a chemical equation in your response.

c) One student's results are given below:

- Concentration of NaOH_{(aq)} = 0.110M

- Volume of undiluted vinegar = 10.00mL

- total volume of diluted vinegar = 100.00mL

- volume of diluted vinegar used in each titration = 20.00mL

- Avg. titre of NaOH_{(aq)} = 15.35mL

Based on these results, calculate the concentration, in mol L^{-1}, of acetic acid in the undiluted vinegar solution.

Step 1

(a) The number of moles of NaOH (*n*) is calculated using equation (1) in which *C* is the concentration and *V* is the volume of solution.

Step 2

One mole of NaOH neutralizes one mole of carboxylic acid. The number of moles of acid is equal to the number of moles of NaOH (*n*). The molar mass of acid (*M*) is calculated using equation (2) in which *m* is the mass of the acid dissolved.

Step 3

The molar mass of the given acid is close to that of the prop...

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