20.0ml of 0. 100M HCI solution in a small beaker is titrated with 0.10M NaOH sol

Question

20.0ml of 0. 100M HCI solution in a small beaker is titrated with 0.10M NaOH solution from a buret. All experiments are carried out at 25°C 2. a) Write the acid-base reaction that occurs during the titration. 2a. b) Calculate the value of the equilibrium constant for the titration reaction in Is it reasonable to assume that this titration reaction goes essentially to completion? Explain. c) Predict the pH of the solution at the equivalence point of the titration (acidic, basic or neutral). Explain your reasoning

Explanation / Answer

a)An acid–base titration is the determination of the concentration of an acid or base by exactly neutralizing the acid or base with an acid or base of known concentration. This allows for quantitative analysis of the concentration of an unknown acid orbase solution.

c)acidic because as the titration of acid and base titration change naoh react with hcI the colour change occur at acidic medium that is use of phenolpthalein indicator

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