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What solution would require the greatest amount of base to be added to bring the solution to neutral pH?
To determine which solution would require the greatest amount of base to reach a neutral pH, you would look for the solution with the lowest initial pH. For example, a strong acid solution, such as hydrochloric acid (HCl) at a low concentration (e.g., pH 1), would require significantly more base to neutralize it compared to a solution with a pH closer to neutral, like a weak acid solution. The greater the acidity (lower pH), the more base is needed to achieve a neutral pH of 7.
If the pH of a solution is 6 would you expect to find more or fewer hydrogen ions than a solution with a pH of 3?
You would expect to find fewer hydrogen ions in the solution with a pH of 6 compared to a solution with a pH of 3. pH is a measure of the concentration of hydrogen ions in a solution, so as the pH value increases, the concentration of hydrogen ions decreases.
If the pH of a solution is 6.2 what would the PO be?
To find the pOH of a solution, you can use the relationship between pH and pOH, which is given by the equation: pH + pOH = 14. If the pH of the solution is 6.2, then the pOH can be calculated as follows: pOH = 14 - pH = 14 - 6.2 = 7.8. Therefore, the pOH of the solution is 7.8.
What is the pH of a solution with H plus equals 7.0 10-7?
The pH of a solution is calculated using the formula pH = -log[H+]. Plugging in the given value of [H+] = 7.0x10^-7, you would get a pH of 6.15 for this solution.
If a solution has a pH of 5 what would it react with to form a salt?
A solution with a pH of 5 would react with a base to form a salt. The base would neutralize the acidic solution, resulting in the formation of a salt and water.
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 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 pH of a 1.45M HNO3 solution?
The pH of a 1.45M HNO3 solution is approximately 0.14. This is because nitric acid is a strong acid that dissociates completely in water to yield H+ ions.
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 a 1.6 10-3 M HNO3 solution?
pH = -log[H+] pH = -log[1.6 × 10-3] pH = 2.8
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 will the pH of 250.0ml of aqueous containing 12.6g nitric acid?
HNO3 is nitric acid with a molecular weight of 63. So 126g would be 2 moles and hence 12.6g =0.2 moles. This is in 0.25 liters so the total molarity is 1000/250 x 0.2 = 0.8 molar. pH = - log10 [H+] so = -log10 0.8 = 0.097 or pH 0.1 rounded.
What is the pH of 2M HNO3?
The pH of a 2M HNO3 solution is approximately 0. This is because nitric acid (HNO3) is a strong acid that fully dissociates in water to release H+ ions, resulting in a highly acidic solution with a low pH value.
What is the pH of a solution that contains 1.32 grams of nitric acid dissolved in 750 milliters of water?
Two steps. Find molarity of nitric acid and need moles HNO3.Then find pH. 1.32 grams HNO3 (1 mole HNO3/63.018 grams) = 0.020946 moles nitric acid ------------------------------------- Molarity = moles of solute/Liters of solution ( 750 milliliters = 0.750 Liters ) Molarity = 0.020946 moles HNO3/0.750 Liters = 0.027928 M HNO3 ----------------------------------finally, - log(0.027928 M HNO3) = 1.55 pH ==========( could call it 1.6 pH )
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 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.
