Chemistry questions and answers. 3. Use your knowledge of molarity and volume to calculate the number of moles of OH in 12.65 mL of a 0.015 M NaOH solution (see Data Analysis section for some hints) Calculate the number of moles of HNO3 that would be needed to completely neutralize 0.025 moles of NaOH 4. 5. Calculate the pH of a 50 mL solution
This means that after the reaction takes places, your solution will contain 0 moles of hydrochloric acid and "0.003203 moles " - " 0.001431 moles" = "0.001772 moles NaOH" At this point, you should be able to say that the "pH" of the resulting solution must be >7 because you're left with a solution that contains a strong base.The example below demonstrates the technique to solve a titration problem for a titration of sulfuric acid with sodium hydroxide. Example 21.18.1 21.18. 1. In a titration of sulfuric acid against sodium hydroxide, 32.20mL 32.20 mL of 0.250M NaOH 0.250 M NaOH is required to neutralize 26.60mL 26.60 mL of H2SO4 H 2 SO 4.pH and pOH Calculations 1) Determine the pH of a 0.00340 M HNO3 solution. 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. 4) If a solution is created by adding water to 2.30 x 10-4 moles of NaOH and 4.50 x 10-6 moles of HBr until the final volume is 1.00 L, what is the pH of this solution?
Calculating pH. To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per liter . The pH is then calculated using the expression: pH = - log [H 3 O +]. Example: Find the pH of a 0.0025 M HCl solution. The HCl is a strong acid and is 100% ionized in water.
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