A 700.0 mL solution with 0.20 moles of ammonia (Kb = 1.8x10-5) is made. Solve for the pH of each solution below after it is added to our initial ammonia solution.
(a) 700.0 mL of pure water.
(b) 700.0 mL of pure water and 0.20 moles of hydrochloric acid.
(c) 700.0 mL of pure water and 0.30 moles of hydrochloric acid.
A 700.0 mL solution with 0.20 moles of ammonia (Kb = 1.8x10-5) is made. Solve for...
For this question, we have a 17 mL solution of 1.7M ammonia, Kb=1.8x10-5 a) What is the initial pH? b) What is the pH when 40 mL of 0.17 M HCl has been added? c) Where was the equivalence point volume? d) What is the pH when 8 mL of HCl has been added?
Calculate the pH for 100. mL of a 0.500 M solution of ammonia, (NH3 Kb=1.8x10-5) being titrated with 0.500 M HCl at the following positions in the titration. i) The initial pH (before any HCl has been added). A. 9.44 B. 10.81 C. 11.48 D. 12.00 E. 11.75
Assume that you are titrating 60.0mL of 0.05 M Ammonia (Kb = 1.8x10^-5) with 0.1 M Hydrochloric Acid. Fill in the following table and explain your answers with calculation. (I really need a thorough table and calculations here, I understand almost nothing of this, please help.) This is all the info I have for the whole question Volume(mL) of HCl added Total volume(mL) [NH3] [NH4+] {H3O+](Fill this in only after equivalence point is reached) pOH pH 0 mL 15 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...
A buffer made with 150.00 mL of 0.20 M formic acid (Ka=1.8x10-4) and 250.00 mL of 0.10 M formate has a final volume of 1.0 L. What is the pH after 6.00 mL of 1.0 M HCL is added to the buffer?
Ka * Kb = Kw = 1.0 X 10-14 A 25.0 ml sample of a 0.100 M solution of aqueo us ammonia is titrated with a 0.125 M solution of HCI. Calculate the pH of the solution after 0.00, 10.0, 20.0, 30.00, and 40.0 mL of acid have been added; Kb of NH3= 1.8 X 10-5 at 25 °C. Hint: First find the moles after each 10.00 ml of acid is added. Then find the concentration after equilibrium is reached.
What is the pH of a solution containing 0.50 M ammonia and 0.50 M ammonium chloride? What will the pH be after 25mL of 0.20 M of hydrochloric acid has been added to 100.0mL of the solution containing the ammonia and ammonium chloride? What will the pH be after 18mL of 0.25 M of lithium hydroxide has been added to 100.0mL of the solution containing the ammonia and ammonium chloride? The ionization constant for ammonia is 1.8x10-5.
What is the pH of a 0.4647 M aqueous solution of ammonia? Kb (NH3) = 1.8x10-5
1) Calculate the pH of a 0.026 M solution of NH4NO3. Kb of NH3= 1.8x10^-5. include both the dissociation and hydrolysis equations in the set up 2)calculate the pH of a 75 ml buffer solution containing 0.20 M of citric acid(C6H8O7, Ka= 3.2x10^-7) and 0.30 M sodium citrate. and what is the pH after adding 3.0 mlbof 1.5 M HCl to the buffer solution in that question? 3) what is the pH of 20.00 ml of 0.40 M nitrous acid(...
Determine whether the compounds below could be used to prepare an buffer solution. ammonia: Kb=1.8x10-5 acetic acid: Ka=1.8x10-5 chlorous acid: Ka=1.1x10-2 calcium hydroxide: pKb>>1 sulfuric acid: Ka1>>1 carbonic acid: Ka=4.3x10-7 Which can and can't be used?