7) The pH of 20 M HNO3 is... (Note: HNO, is a strong acid) a) .20...
Nitric acid, HNO3, is a strong acid What is the pH AND [ OH-] of a 0.050 M solution of HNO3 at 25 degrees
Calculate the pH of each of the following strong acid solutions. (a) 0.00851 M HCl pH = (b) 0.714 g of HNO3 in 18.0 L of solution pH = (c) 62.0 mL of 4.90 M HCl diluted to 3.00 L pH = (d) a mixture formed by adding 55.0 mL of 0.00326 M HCl to 46.0 mL of 0.00896 M HNO3 pH =
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base Weak base, strong acid pH less than 7 pH equal to 7 pH greater than 7 B. A 56.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 28.0 mL of KOH. C. Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8 x 10^-5) with 0.20 M HNO3....
17. The density of nitric acid (which is HNO3 in water) is 1.42 g/mL. The m/m% of HNO, in nitric acid is 69% m/m. How many grams of HNO3 are in 1 mL of nitric acid? a) 0.99g b) 99g c) 2.1g d) 0.021 g e) 0.49g
Tutored Practice Problem 17.3.3 COURTS TOWARDS GRADE Calculate pH for a weak base/strong acid titration. Close Problem Determine the pH during the titration of 31.9 mL of 0.388 M ammonia (NH3, Kb - 1.8*10*) by 0.388 M HNO, at the following points. (a) Before the addition of any HNO3 (b) After the addition of 12.3 mL of HNO, (c) At the titration midpoint (d) At the equivalence point (e) After adding 45.6 mL of HNO3 HP OfficeJet 4650 series Check...
Calculate the pH of a strong acid solution formed by mixing 83.3 mL of 0.0297 M HBrO4 with 77.2 mL of 0.129 M HNO3. a) The pH of this solution is 0.8. b) The pH of this solution is 1.1. c) The pH of this solution is 0.5. d) The pH of this solution is 4.4. e) The pH of this solution is 1.9.
calc pH of ea strong acid solution (express in 3 decimals) a. 2.11×10−2 M HNO3 b. 0.220 g of HClO3 in 1.80 L of solution c. 10.00 mL of 2.00 M HCl diluted to 0.530 L . d. mixture formed by adding 60.0 mL of 2.5×10−2 M HCl to 160 mL of 1.0×10−2 M HI.
Calculate pH for a strong acid/strong base titration. Determine the pH during the titration of 31.0 mL of 0.342 M HNO3 by 0.342 M NaOH at the following points: (a) Before the addition of any NaOH (b) After the addition of 15.5 mL of NaOH (c) At the equivalence point (d) After adding 40.0 mL of NaOH
Calculate the pH of each of the following strong acid solutions. 4.16×10−2 M HNO3. 0.250 g of HClO3 in 1.50 L of solution. 15.00 mL of 1.10 M HCl diluted to 0.520 L .
10-7 moles of the strong acid HNO3 are added to 1 Lt of distilled water at 25 oC. What is the pH of the solution? Assume that activity coefficients are unity. Show all the assumptions you make.