An aqueous solution at 25 ∘C is 12.7 % HNO3 by mass and has a density of 1.059 g/mL. What is the pH of the solution?
Use the Henderson-Hasselbalch equation to determine the moles of H+added to the solution, resulting in a pH=7.24
An aqueous solution at 25 ∘C is 12.7 % HNO3 by mass and has a density...
An aqueous solution at 25 °C is 10.8% HNO3 by mass and has a density of 1.044 g/mL. What is the pH?
An aqueous solution at 25 °C is 13.0% HNO, by mass and has a density of 1.042 g/mL. What is the pH of the solution? pH =
at 20 degree Celsius an aqueous solution of HNO3 that is 35.0% HNO3 by mass has a density of 1.21g/mL A). how many grams of HNO3 are present in 2.73 L of this solution? B.) what is the volume of this solution will contain 502 g HNO3?
Introductory chemistry 20 A nitric acid solution containing 71.0% HNO3 (by mass) has a density of 1.42 g/mL. ow many moles of HNO, are present in 2.36 L of this solution? b) Determine the molarity of the acid.
Calculate pH of a weak acid/conjugate base buffer solution. 1. a) Calculate the pH of 650. mL of a 0.211-M solution of acetic acid before and after the addition of 0.123 mol of potassium acetate. pH befor addition = pH after addition = 1 b) Calculate pH of a weak base/conjugate acid buffer solution. A 0.190-M aqueous solution of C2H5NH2 (ethylamine) has a pH of 11.9. Calculate the pH of a buffer solution that is 0.190 M in C2H5NH2 and...
Question 12 Determine the molarity of a 0.919 m aqueous solution of HNO3. The density of the solution is 1.35 g/mL
Weak-Acid Strong-Base Titrations. These next questions relate to a 25 mL aliquot of 0.35 M acetic acid (Ka = 1.77 x 10) that is titrated with 0.20 M potassium hydroxide (KOH). (f) What is the pH of the acetic acid solution before the titration begins? (g) What is the pH after 14 mL of 0.20 M KOH has been added to the solution? Use the Henderson-Hasselbalch equation. (h) What is the pH at the equivalence point?
An aqueous solution of MgCl2 that is 27.5% (mass%) and has a solution density of 1.25 g/mL. MgCl2 has a molar mass of 95.211 g/mol. What is the molarity of this MgCl2 solution?
1a. An aqueous solution has a Molarity of 1.632 M. The density of the solution is (1.150x10^0) g/mL and the solute has a molar mass of (1.33x10^2) g/mol. What is the molality of this solution? 1b. An aqueous solution has a mass percent of solute of 18.4%. The density of the solution is (1.400x10^0) g/mL and the solute has a molar mass of (1.77x10^2) g/mol. What is the molality of this solution? 1c. An aqueous solution has a molality of...
c) Calculate the pH if 95 ml of 10.0M HC (ag) is added to 200.0 ml of this buffer. For full creds, show your work in detail. (4) aj Calculate the pH if 9.5 mL of 10.0 M NaOH (ag) is added to 200.0 mL ofa freshly prepared solution of this buffer. For full credit, show your work in detail (4) e) You should see from the calculations that this buffer is better able to buffer against added acid than...