16. A solution contains 4.25 g of ammonia (NH3) in 350 ml of solution. Electrical conductivity...
The pH of an ammonia, NH3, solution is 9.50. The Kb for ammonia is 1.78 x 10-5?a. Write the balanced chemical equation for the reaction of ammonia with water. b. Write the term for the Kc for this reaction. c. What is the concentration in mol L-1 of ammonia added to water to make this solution at pH 9.5?
A solution of household ammonia is 3.0 % NH3(aq) and has a density of .98 g/ml. What is the molar concentration of the NH3(aq)? Given that the Kb for NH3(aq) = 1.8x10‒5, what is the predicted pH of this solution? Thank you in advance
- An aqueous solution contains 0.319 M ammonia (NH3). How many mL of 0.318 M nitric acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 9.700. --- mL
Exercise 16.34 A particular household ammonia solution (d = 0.97 g/mL) is 6.8% NH3 by mass. How many milliliters of this solution should be diluted with water to produce 625 mL of a solution with pH = 11.65? Express your answer using two significant figures.
An aqueous solution contains 0.483 M ammonia (NH3). How many mL of 0.206 M hydroiodic acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 9.090? mL
a) What is the pH of a solution that consist of 0.20 M ammonia, NH3, and 0.20 M ammonium choride, NH4Cl? (Kb for ammonia is 1.8 x 10-5) b) 1.25 g of benzoic acid (C6H5CO2H) and 1.25 g of sodium benzoate (NaC6H5CO2) are dissolved in enough water to make 250 mL solution. Calculate the pH of the solution using the Handerson-Hasselbach equation (Ka for benzoic acid is 6.3 x 10-5). c) What is the pH after adding 82 mg of...
An aqueous solution contains 0.381 M ammonia (NH3). How many mL of 0.215 M hydrochloric acid would have to be added to 250 mL of this solution in order to prepare a buffer with a pH of 9.090?
A rigid container initially contains only 0.25 mol of NH3 (g) in a 5.0 L volume. We introduce 0.20 mol of HCI (g) at 25 °C. a. Write the chemical equation for this reaction assuming that it forms one product. b. Calculate the final pressure in the container after the reaction in a. is complete If some of this product were added to water, what would happen to the pH of solution relative to pure water? c. Instead of the...
Commercial concentrated aqueous ammonia is 28.0% NH3 by mass. What volume of this solution contains 100.g of NH3? (Density = 0.900 g/mL) 0 397 ml O 357 ml 0 28.0 mL 25.2 mL 321 ml 595 mL
An aqueous solution is 0.500% by mass ammonia, NH3, and has a density of 0.996 g/mL. The molality of ammonia in the solution is m.