1) A 75.0-mL volume of 0.200 M NH3 ( K b=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 23.0 mL of HNO3. 2)A 52.0-mL volume of 0.35 M CH3COOH ( K a=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 21.0 mL of NaOH. Determine the pH of the solution after the addition of 200.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4. A) 3.34 B) 3.57 C) 3.46 D) 2.89 E) 3.63. B. First thing first, calculate the total volume of the resulting solution. #V_"total" = "100.0 mL + 50.0 mL + 100.0 mL"# #V_"total" = "250.0 mL"# Now, you are dealing with two strong acids that ionize completely in aqueous solution. Both nitric acid and hydrochloric acid produce hydronium cations in #1:1# mole ratios, so you know that Explanation: We use the pH equation, which states that. pH = −log[H +] or pH = − log[H 3O+] It is the same equation anyways, as water can dissociate two ways. Since the hydrochloric acid has a concentration of 0.34 M, that must mean that the concentration of hydronium (H 3O+) ions is also 0.34 M, i.e. there exists 0.34 moles of hydronium Some chemists and analysts prefer to work in acid concentration units of Molarity (moles/liter). To calculate the molarity of a 70 wt. % nitric acid the number of moles of HNO 3 present in 1 liter of acid needs to be calculated. Knowing the density of the acid to be 1.413 g/mL, we can calculate the weight of 1 L of 70% HNO 3 to be 1413 A. A 75.0- mL volume of 0.200 M NH3 ( Kb=1.8×10−5 ) is titrated with 0.500 M HNO3 . Calculate the pH after the addition of 11.0 mL of HNO3 . Express your answer numerically. B. A 52.0- mL volume of 0.35 M CH3COOH ( Ka=1.8×10−5 ) is titrated with 0.40 M NaOH . Calculate the pH after the addition of 29.0 mL of NaOH . Express your answer Calculate the pH for the strong acid/strong base titration between 50.0 mL of 0.100 M HNO 3 (aq) and 0.200 M NaOH (titrant) at the listed volumes of added base: 0.00 mL, 15.0 mL, 25.0 mL, and 40.0 mL. To calculate pH, remember that the pH scale goes from 0 to 14 with numbers below 7 being acidic and numbers above 7 being basic. If you are doing chemistry in a lab, you will need to determine the concentration by finding the moles per unit of volume (m/v or M). If you are doing a chemistry problem, look at the equation to identify the The pH of pure water will thus be. pH = −log([H3O+]) pH = −log(10−7) = 7. Now, let's assume that you're working with a 1.0-L solution of pure water and you add some 10−8M hydrochloric acid solution. To keep calculations simple, let's assume that the volume remains unchanged upon adding this hydrochloric acid solution. 1. A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Kb, NH3 = 1.8 × 10−5. Determine the pH of the solution at each of the following points in the titration: (a) Calculate the volume (mL) of HCl required to reach the equivalence point. Plot the points from part (c) on a graph. The total [H +] from the two acids is 0.51 M and [OH - ] from NaOH is 0.62 M. Therefore, 0.51 moles per liter of H + will react with 0.51 moles per liter of OH - to form water. That leaves a 0.11 M NaOH solution. The pOH of a 0.11 M NaOH solution is 0.96 pOH units, and the pH is 13.04 pH units. Calculate the pH of 0.100 L of a buffer solution that is 0.20 M in HF (Ka = 3.5 x 10-4 ) and 0.47 M in NaF. Express your answer using three significant figures. pH = 3.83 Part B What is the pH after adding 0.003 mol of HNO3 to the buffer described in Part A? Express your answer using three significant figures. Calculate the pH from the equation: pH = -log[H +] = -log[0.001] = 3. Then use the formula which shows the relationship between pH and pOH: pH + pOH = 14. and calculate pOH as: 14 - pH = 14 - 3 = 11 How to Calculate pH and [H+] The equilibrium equation yields the following formula for pH: pH = -log 10 [H +] [H +] = 10 -pH. In other words, pH is the negative log of the molar hydrogen ion concentration or the molar hydrogen ion concentration equals 10 to the power of the negative pH value. It's easy to do this calculation on any scientific A- 8. The samples of nitric and acetic acid shown here are both titrated with a 0.100 M solution of NaOH (aq).Determine whether each of the following statements concerning these titrations is true or false. (a) A larger volume of NaOH (aq) is needed to reach the equivalence point in the titration of HNO3. (b) The pH at the equivalence point in qjmdqj.

calculate ph of hno3