An Erlenmeyer flask contains 25.00 mL of 0.10 M HCl. What is the pH of the solution?

Chemistry

2 answers:

Eduardwww [97]3 years ago

6 0

Answer:

The pH of the solution is 1.

Explanation:

Concentration of HCl solution = 0.10 M

$HCl\rightarrow H^++Cl^-$

1 mole of HCl gives 1 mole of $H^+$ ions.

$[HCl]=[H^+]=0.10 M$

The pH of the solution is defined as negative logarithm of $H^+$ ions in the solution.Mathematically written as

$pH=-\log[H^+]$

$pH=-\log[0.10 M]=1$

The pH of the solution is 1.

max2010maxim [7]3 years ago

4 0

C=0.10 mol/l

pH=-lg[H⁺]

HCl = H⁺ + Cl⁻

pH=-lgc

pH=-lg0.10=1.0

pH=1.0

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A chemist must prepare of hydrochloric acid solution with a pH of at . He will do this in three steps: Fill a volumetric flask a

Eva8 [605]

Answer:

1.7 mL

Explanation:

<em>A chemist must prepare 550.0 mL of hydrochloric acid solution with a pH of 1.60 at 25 °C. He will do this in three steps: Fill a 550.0 mL volumetric flask about halfway with distilled water. Measure out a small volume of concentrated (8.0 M) stock hydrochloric acid solution and add it to the flask. Fill the flask to the mark with distilled water. Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits.</em>

Step 1: Calculate [H⁺] in the dilute solution

We will use the following expresion.

pH = -log [H⁺]

[H⁺] = antilog - pH = antilog -1.60 = 0.0251 M

Since HCl is a strong monoprotic acid, the concentration of HCl in the dilute solution is 0.0251 M.

Step 2: Calculate the volume of the concentrated HCl solution

We want to prepare 550.0 mL of a 0.0251 M HCl solution. We can calculate the volume of the 8.0 M solution using the dilution rule.

C₁ × V₁ = C₂ × V₂

V₁ = C₂ × V₂/C₁

V₁ = 0.0251 M × 550.0 mL/8.0 M = 1.7 mL

3 0

2 years ago