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pH = -log[H+]

pH = -log[1.6 × 10-3]

pH = 2.8

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What is the pH of a 0.6 M HNO3 solution?

The pH of a 0.6 M HNO3 solution is approximately 0.23. This is because nitric acid is a strong acid that completely ionizes in solution, resulting in a high concentration of H+ ions that lower the pH.


What is the pH and pOH of a 0.0067M HON3 solution?

Since HNO3 is a strong acid, it completely dissociates in solution. HNO3 -> H+ + NO3-. Therefore, the concentration of H+ ions is the same as the concentration of the HNO3 solution, 0.0067M. pH = -log[H+] = -log(0.0067) ≈ 2.18. pOH = 14 - pH ≈ 11.82.


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What is the pH of a 1.45M HNO3 solution?

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What is the concentration of HNO3 in a solution with pH3.4?

The concentration of HNO3 in a solution with pH 3.4 is approximately 3.98 x 10^-4 M. This is calculated using the formula pH = -log[H+], where [H+] is the hydrogen ion concentration in mol/L. For nitric acid (HNO3), one mole of HNO3 produces one mole of H+ in solution.


What is the pH of 15 mL of 0.0045 M HNO3?

pH = - log10 [H+], where [H+] is the molar concentration of hydrogen ions. HNO3 is a strong acid and dissociates completely in water so a 5 M solution of HNO3 would have a concentration of hydrogen ions of 5M also. So, pH = -log10[5] = -0.699 which indicates an extremely strong acid.


What is the pH of 2M HNO3?

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If hno3 is added to water how does pH- change?

If nitric acid (HNO3) is added to water, it decreases the concentration of hydroxide ions in solution. This is because nitric acid semi-strongly dissociates in water, following this chemical reaction: HNO3(aq) + H2O(l)-->NO3-(aq) + H3O+(aq) The hydronium ions that are created in this reaction then react quickly with the hydroxide ions in the water, as shown in this chemical equation: H3O+(aq) +OH-(aq) --> 2H2O(l) This results in fewer hydroxide ions existing in solution.


What is hydrogen ion concentration of 0.5 HNO3?

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What is the pH of an acidic solution?

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