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How many millimoles of HNO3 are present at the start of a titration?
The number of millimoles of HNO3 present at the start of a titration will depend on the initial concentration and volume of the HNO3 solution. To calculate millimoles, you can multiply the concentration of HNO3 in moles per liter by the volume of the solution in liters.
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.
What is the molarity of nitric acid?
The molarity of nitric acid, HNO3, can vary depending on the concentration of the solution. For example, a 1 M solution of nitric acid would contain 1 mole of HNO3 per liter of solution. It is important to know the concentration or volume of the solution to determine the molarity of nitric acid.
What is hydrogen ion concentration of 0.5 HNO3?
A 0.5 M solution of HNO3 will have a hydrogen ion concentration of 0.5 moles per liter. This is because each molecule of HNO3 ionizes to produce one hydrogen ion in solution.
What is the pH of a 0.01 M solution of the acid HNO3 in water?
- log(0.01 M HNO3) = 2 pH =====
How many millimoles of HNO3 are present at the start of a titration?
The number of millimoles of HNO3 present at the start of a titration will depend on the initial concentration and volume of the HNO3 solution. To calculate millimoles, you can multiply the concentration of HNO3 in moles per liter by the volume of the solution in liters.
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.
What is the molarity of nitric acid?
The molarity of nitric acid, HNO3, can vary depending on the concentration of the solution. For example, a 1 M solution of nitric acid would contain 1 mole of HNO3 per liter of solution. It is important to know the concentration or volume of the solution to determine the molarity of nitric acid.
What is hydrogen ion concentration of 0.5 HNO3?
A 0.5 M solution of HNO3 will have a hydrogen ion concentration of 0.5 moles per liter. This is because each molecule of HNO3 ionizes to produce one hydrogen ion in solution.
Which substance increase h ion concentration in a solution?
acids such as HCl, H2SO4 HNO3 etc
What is the pH of a 0.01 M solution of the acid HNO3 in water?
- log(0.01 M HNO3) = 2 pH =====
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 does 15 M HNO3 mean?
15 M HNO3 indicates a solution of nitric acid with a concentration of 15 moles per liter. This solution is highly acidic and can be used for various chemical reactions and laboratory purposes. The M signifies molarity, a measurement of concentration.
What is HNO3 in water?
HNO3 does not react with water.It become diluted with water.
What is the molarity of OH- in an aqueous solution that is 0.34 M HNO3?
Since HNO3 is a strong acid that completely dissociates in solution, the concentration of H+ ions is equal to the concentration of the acid, which is 0.34 M. The concentration of OH- ions in water is 1.0 x 10^-14 M, therefore, the molarity of OH- ions in the solution is also 1.0 x 10^-14 M.
What is the pH of a 1.6 10-3 M HNO3 solution?
pH = -log[H+] pH = -log[1.6 × 10-3] pH = 2.8
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.
