For the titration of 250 ml of 0100 m hclaq with 0225 m...

For the titration of 25.0 mL of 0.100 M HCl(aq) with 0.225 M NaOH(aq). a. Calculate the initial pH of the 0.10 M HCl(aq), before any NaOH is added b. What volume of NaOH in mL is required to reach the equivalence point in the titration?

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00:01 Of 25 milliliter of 0 .1 molar of hydrochloric acid with 0 .225 molar of sodium chloride.

00:10 Calculate initial ph of the 0 .1 molar of hydrochloric acid.

00:18 So what we know is that we have a 0 .1 molar of hydrochloric acid.

00:27 So this tells us that hydrochloric acid dissociate to form hydrogen ion and sodium ion.

00:37 So 0 .1 molar of hydrochloric acid produce 0 .1 molar of proton or hydrogen ion.

00:46 So before the addition of sodium hydroxide, the concentration of the hydrogen ion is 0 .1 molar.

00:57 So we can calculate the ph, negative log concentration of hydrogen ion, negative log of 0 .1 equals 1.

01:18 So before titration, the ph of the 0 .1 molar of hydrochloric acid is 1.

01:28 Second question, now what volume of sodium hydroxide in milliliter is required to reach equilibrium point in the titration? so we have to know the equation hcl plus naoh.

01:46 So sodium hydroxide, they neutralize each other.

01:52 So the equation is water and nacl.

01:59 So we can tell that after neutralize each other, they produce sodium chloride and water.

02:06 So the molar ratio between hydrochloric acid and sodium hydroxide is a 1 to 1 ratio.

02:15 Now let's first of all see how much hydrochloric acid that we have.

02:23 So now the mole of hydrochloric acid equals the volume times the concentration...

Question

For the titration of 25.0 mL of 0.100 M HCl(aq) with 0.225 M NaOH(aq). a. Calculate the initial pH of the 0.10 M HCl(aq), before any NaOH is added b. What volume of NaOH in mL is required to reach the equivalence point in the titration?

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