What Is The Ph Of A 0.056 M Hno3 Solution

What Is The Ph Of A 0.056 M Hno3 Solution?

You should get an answer of 1.25. Okay that’s the Ph.Jul 12 2017

What is the pH of a 0.0045 M HNO3 solution?

The solution with [H+] = 0.0045 M will have a pH of 2.35.

What is the pH of a 0.008 M solution of HNO3?

You’re going to get 2.1. Okay so that’s the pH of the solution that’s labeled.

What will be the pH of 0.000001 M HNO3 solution?

Explanation: log10{0.0001} = log10(10−4)=−4 by definition of the log function. Thus pH = 4 and necessarily pOH=10 .

What is the pH of a 0.400 M HNO3 solution?

This problem has been solved!

(b) The measured pH of a 0.400 M HNO3 solution at the same temperature is 0.538.

What is the pH of HNO3?

1.08

pH of Common Acids and Bases
Acid Name 100 mM
HNO3 nitric acid 1.08
H3PO4 orthophosphoric acid 1.63
H3AsO4 arsenic acid 1.70
H2SeO3 selenous acid 1.90

What is the pH of 0.6 M HNO3 solution?

0.222

The pH of 0.6 M Nitric acid is 0.222 which is a highly acidic solution.

How do you find the pH from molarity of HNO3?

1) Determine the pH of a 0.00340 M HNO3 solution. pH = -log[H+] = -log(0.00340) = 2.47 2) Determine the pOH of a 0.00340 M HNO3 solution. 3) Determine the pH of a 4.30 x 10-4 M NaOH solution.

What is the pH of 0.50 M HNO3?

Question: The pH of a 0.50 M HNO3 solution is 1.83.

What is the pH of 0.1 M HNO3?

1.0

The concentration of H₃O⁺ in a strong acid solution is therefore equal to the initial concentration of the acid. For example a solution of 0.1 M HNO₃ contains 0.1 M H₃O⁺ and has a pH of 1.0.

What is the pH of a 3m solution of HNO3?

1.6021

From the concentration of nitric acid calculate the concentration of hydrogen ions. Use the concentration of hydrogen ions to calculate the pH of the solution. Thus the pH of the solution is 1.6021.

What is the pH of 0.001 M HNO3 How much did one drop of HNO3 cause the pH of water to change?

How much did one drop of HNO3 cause the pH of water to change? Water has a pH of 7. If 0.1 mL (about one drop) of 1.0 M HNO3 is added to 100 mL of water the result is a solution with a concentration of 0.001 M HNO3.

What is the pH of a 0.100 M HCN solution?

pH of a 0.1M HCN solution is 5.2 .

What is the pH of a 1.00 M solution of HNO2?

Question: Question 1: Calculate the pH of a solution that is 1.00 M HNO2 and 1.00 M NaNO2. My answer: ph = 3.40 (my work attached in the photo.

Is HNO3 an acid?

HNO3 is a potent acid a base a nitrating agent and a heavy oxidising agent at times. In the presence of a stronger acid it serves as a base.

How do you go from M to pH?

To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per liter (molarity). The pH is then calculated using the expression: pH = – log [H3O+].

What is the pH of a 0.00001 molar HCl solution?

– We know that HCl dissolves to give protons and chloride ions. The dissociation reaction in aqueous medium can be given as below. Thus the pH of the solution will be 8.

How do you find the pH of barium hydroxide?

pH=−log10([H+]=5.0×10−14)=13.30 .

What is the pH of a 0.01 M solution of KOH?

12
The `pH` of `0.01 (M) KOH` is `12` if the temperature of the given `KOH` solution is increased – YouTube.Jan 19 2020

What is the pH of a 1.4 M solution of HClO4?

-0.15

The pH of a 1.4 M solution of HClO4 is -0.15. Perchloric acid or HClO4 is a strong acid.

What is the pH of a 0.20 M nitric acid HNO3 solution?

0.70

Since a complete dissociation occurs for a strong acid such as nitric acid the concentration of the hydronium ion is also equal to 0.20 M (the same as the concentration of nitric acid). With this we can now calculate the pH value of the solution. The pH of the solution is equal to 0.70.

0.0013M 2.89.

What is the pH of a 0.50 M C5H5N pyridine solution?

Calculate the pH of a 0.50 M solution of pyridine (C5H5N Kb= 1.7 x 10-9). PH= 14 – 4.5 = 9.5 Basic!

What is the pH of 0.50 m?

Solved The pH of 0.50 M acetic acid is 2.52.

The pH = 11.3 .

What is the pH of 0.1 M HF?

3.45

An aqueous solution containing 0.1M HF and 0.1 M KF has a pH of 3.45.

What is the pH of a 1.0 M solution of a strong acid?

pH-values for very strong acids are easy to calculate because the concentration of H+ (or H3O+) is identical to the concentration of HCl in the solution. Thus with pH = -log concentration of H+ the 1 M solution of HCl will give the pH of -log 1 or 0 (Zero) because 10 ^0 = 1.

What would be the pH of a 0.01 M solution of a strong acid?

Hence the answer is – option (d) – the pH of 0.01 M solution of HCl is 2. =>pOH = 14 – pH.

What is the pH of a 0.04 M KOH solution?

Therefore 0.04 M KOH has a pH of 12.6.

What is the pH of a 0.0235 m HCl solution?

1.629 2

pH = -log[H+] = -log(0.0235) = 1.629

2) What is the pOH of a 0.0235 M HCl solution?

What is the pH of a 0.0067 M potassium hydroxide solution?

\$11.83

Molar concentration of \${K_w}\$ is \$1 times {10^{ – 14}}\$. Molar concentration of \$[O{H^ – }]\$ ion is \$6.7 times {10^{ – 3}}M\$. Hence pH value of \$0.0067M\$ \$KOH\$ solution is \$11.83\$.

What is the pOH of HNO3?

14 − pH

So now we know that pOH =14 − pH.

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