250 ml volume of a mixture of 0.8g of NaHCO3 and 0.2g of NaOH in water. Take 50 ml of this mixture and titrate with o.1 N of HCI. Calculate the volume of acid? ( Atomic weight = Na=23, H=1,O =16, CI =35 , C=12, N= 14) * 30 ml. 5 ml. 25 ml. 10 ml. O 45 ml.
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- What is the pH of the ethanoic acid solution CH3COOH 0.15 M with Ka = 1.8 × 10-⁵? b) What will be the pH when in 82 liters of 0.15 M solution of this acid we add 82 grams of sodium ethanoate CH3COONa?if all the N in 10.0 mmols urea, CO(NH2)2, is converted to NH4HSO4, and if, with excess NaOH, the NH3 is evolved and caught in 50.0 mL of HCl (1.00 mL = 0.03000 g CaCO3), what volume of NaOH (1.00 mL = 0.3465 g H2C2O4. H2O) would be required for complete titration? using Kjeldahl's Methoda) 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) = 15.35mLBased on these results, calculate the concentration, in mol L-1, of acetic acid in the undiluted vinegar solution.
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