Answer:
Answers are in the explanation
Explanation:
a. The statments are:
The titration process is based on a chemical reaction. <em>TRUE. </em>A titration is the chemical reaction between an acid and a base.
The pH of the solution at the equivalence point is 7. <em>TRUE. </em>In a titration of strong acid with strong base the equivalence point is 7
At the endpoint, the pH of solution is 10 and the color of solution is pink. <em>FALSE</em>. The endpoint in a strong acid - strong base titrationmust be near to equivalence point at pH = 7.
At the beginning of the titration process, the pH of the solution increases rapidly. <em>FALSE. </em>At beginning of a titration, the pH of the solution increases slowly.
The chemical reaction involved in an acid-base titration is a neutralization reaction. <em>TRUE. </em>In the reaction, you are neutralizing an acid (HCl) with a base (NaOH)
Before any base is added to the solution, the pH of the solution is high. <em>FALSE. </em>The addition of a base increases pH that is, in the beginning, low.
In a titration process, the endpoint is reached before the equivalence point. <em>FALSE. </em>In a titration process, the endpoint is reached in the equivalence point
The pH of the solution changes very slowly at the equivalence point. <em>FALSE. </em>At the equivalence point, the pH changes rapidly.
b. For the reaction
NaOH + HCl → H₂O + NaCl
As the reaction is 1:1 and molarity of both solutions are the same, additions < 100mL of NaOH will stay before the equivalence point, equivalence point will be in 100mL and additions > 100mL of NaOH will stay after the equivalence point.
The conditions are:
10.0mL of 1.00 M NaOH before the equivalence point
150 mL of 1.00 M NaOH after the equivalence point
5.00 mL of 1.00 M NaOH before the equivalence point
50.0 mL of 1.00 M NaOH before the equivalence point
200 mL of 1.00 M NaOH after the equivalence point
I hope it helps!
