0
The pH of a 2.0 M solution of HNO3 would be approximately 0. This is because nitric acid (HNO3) is a strong acid that dissociates completely in water to release H+ ions, causing a high concentration of H+ ions in the solution and a low pH value.
pH = -log [H+ ion concentration]
HNO3 is a strong acid, and because it is strong you can just plug 2.0M in for the H+ ion concentration and solve.
If it were a strong base, you would take the answer you got for the above problem as your pOH instead of pH. pOH+pH=14. This method only works for strong acids or bases.
Since each NaOH molecule contains only one hydroxide ion, the normality of NaOH is equal to its molarity. Therefore, 1.0 N of NaOH is the same as 1 M.
Add your answer:
Earn +20 pts
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 of a 0.01 M solution of the acid HNO3 in water?
The pH of a 0.01 M solution of HNO3 would be around 2. Negative logarithm of the hydrogen ion concentration (10^-2) will give a pH value of 2 for the solution.
What is the pH of a 1.6 10-3 M HNO3 solution?
The pH of a 1.6x10^-3 M HNO3 solution is approximately 2.8. This is calculated by taking the negative logarithm (base 10) of the concentration of the hydrogen ions in the 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 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 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 of a 0.01 M solution of the acid HNO3 in water?
The pH of a 0.01 M solution of HNO3 would be around 2. Negative logarithm of the hydrogen ion concentration (10^-2) will give a pH value of 2 for the solution.
What is the pH of a 1.6 10-3 M HNO3 solution?
The pH of a 1.6x10^-3 M HNO3 solution is approximately 2.8. This is calculated by taking the negative logarithm (base 10) of the concentration of the hydrogen ions in the 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 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 a solution that contains 1.32 grams of nitric acid dissolved in 750 milliters of water?
To calculate the pH of the solution, you first need to determine the concentration of nitric acid in moles per liter. Then you can calculate the pH using the formula for pH: pH = -log[H+]. Given the amount of nitric acid and volume of water, you can find the pH.
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 the solution formed by completely neutralizing 50 milliliters of 0.1 m hno3 with 50 milliliters of 0.1 m naoh at 298 k?
The reaction between HNO3 (acid) and NaOH (base) results in the formation of water and a salt, NaNO3. Since both the acid and base are of equal concentration and are completely neutralized, the resulting solution would be a neutral solution with a pH of 7.
How many moles of hno3 are needed to prepare 5.0 of a 2.0 m solution of hno3?
10
What is the molarity of HNO3 if 20.0 ml of the solution is needed to exactly neutralize 10.0 ml of a 1.67 M NaOH solution?
The reaction between HNO3 and NaOH is a 1:1 molar ratio. This means that the moles of HNO3 required to neutralize the NaOH is the same as the moles of NaOH. Given that 20.0 ml of HNO3 is needed to neutralize 10.0 ml of a 1.67 M NaOH solution, the molarity of the HNO3 solution is twice the molarity of the NaOH solution, which is 3.34 M.
What is the molarity of a solution dissolve 0.31 grams of HNO3 in 300ml of water?
The molarity of the solution would be 0.1 M. This is because you need to calculate the number of moles of HNO3 first, which is 0.005 moles, and then divide by the volume of the solution in liters (0.3 L) to get 0.1 M.
What would be pH of a 0.00884 M solution of HNO3?
HNO3 is a strong acid, which means it dissociates completely. This means you don't have to set up an equilibrium scenario; you can just go with the given molarity as also being the concentration of hydrogen ions [H+]. So, pH = -log(0.00884), which is about 2.05.
