What is the pH of a solution of 1.00L of water with 0.0720 moles of HNO3 in it
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What is the pH of a solution of 1.00L of water with 0.0720 moles of HNO3...
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What is the pH of a solution of 1.00L of water with 0.0973 moles of NaOH in it ?
What is the pH of 1.00L of an ammonia/ammonium, NHz/NH4+, base buffer solution containing 0.35M NH; and 0.35M NH,* after 0.030 moles of the strong acid, HNO3, are added (NHz Ky - 1.8 x 10-$)? O pH = 5.2 - 7.2 O pH = 9.2 pH - 12
A 1.00L buffer solution is formed by adding 0.250 moles of KOH (aq) to 0.300 moles of HA. The Ka for HA = 3.1 x 10-5. A. What is the initial pH of the buffer? B. What will pH be after the addition of 0.0500 moles of H3O+? C. 10ml of a 3.5 M solution of NaOH are added to the buffer. What is the resulting pH?
How many moles of NH3 are required in a 1.00L solution to create a buffer with a pH of 8.81 if the solution contains 0.64 moles of NH4Cl? Kb NH3 = 1.8 x 10-5?
How many moles of HClO are required in a 1.00L solution to create a buffer with a pH of 7.22 if the solution contains 0.39 moles of NaClO? Ka HClO = 3.0 x 10-8?
What is the pH after 0.29 moles of NaOH is added to a 1.00L buffer containing 1.00 moles of NH3 and 1.00 moles NH4Cl ? Kb NH3 = 1.8 x 10-5
2. A 1.00L buffer solution is 0.150M HCOOH and 0.350M HCOOLi. A) What is the pH of the buffer? B) What will be the pH after addition of 100.mL of 0.100M HCl solution? Ka of HCOOH = 1.8x104 ( 2 Mar
If 1.00L of water is added to 3.00 L of a 6.00M solution of HCl, what is the new molarity of the acid solution?
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.