Calculate the equilibrium concentrations and pH of the following:
a) 0.58 M HF (Ka=6.8x10^-4)
b)0.75 M NH3 (Kb=1.76x10^-5)
Calculate the equilibrium concentrations and pH of the following: a) 0.58 M HF (Ka=6.8x10^-4) b)0.75 M...
calculate the pH and % ionization of 0.0200 M HF (Ka=6.8x10^-4)
What is the pH of 44.3 ml of a solution which is 0.26 M in NaF and 0.33 M in HF? For HF use Ka=6.8x10^-4
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...
Consider 0.10 M solutions following acids: HF, Ka = 6.8x10-4 HIO, K2 = 2.3x10-11 HC7H502, Ka = 6.3x10-5 HCOOH, K = 1.8x10-4 Which of the following statements is true? HC7H5O2 has the lowest pH and the largest percent dissociation. HF has the highest pH and the largest percent dissociation. HCOOH has the lowest pH and the largest percent dissociation. HIO has the highest pH and the smallest percent dissociation. HF has the lowest pH and HIO has the largest percent...
HF is an acid with Ka=6.8x10-4. A sample of HF with an approximate concentration of 0.10M is titrated with strong base. What will be the pH at the equivalence point?
(15 pt) 8. Calculate the pH and % ionization of 0.0200 M HF (K= 6.8x10")? What is the pH of a buffer that is 0.300 M HF (K = 6.8x10*) and 0.500 M KF?
Calculate the pH of a 0.353 M aqueous solution of hydrofluoric acid (HF, Ka 7.2x10 t) and the equilibrium concentrations of the weak a and its co base. pH HF equilibrium F leg brium M.
Chem II Common Assignment: Equilibrium and Buffers 1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak...
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF) 7.2x10-4; Ka ([Al(H20).]+)7.9x10-6; Ka (H3PO4)=7.5x10-2: Ka (HPO42-) =3.6x10-13; Ka (HCI)=Huge; Ka(Na+)=tiny; Ka(Cl-)tiny; Kb(NH3)=1.8x10-5; Kw=1x10-14 1) Calculate the pH of aqueous 0.25M HCl and 0.25M HF solutions. 2) Complete the following tables for aqueous solutions of conjugate acid-base pKa pKb Kb 1.3x10-4 35 3) Complete the following table for aqueous solutions DHL TH+) OH) pOH 1x102 4) Calculate the pH of aqueous 0.15M Ba(OH)2 and...
the effective pH range of the KF/HF (Ka=6.8x10^-4) buffer is? a) 2.2-4.2 b)1.2-4.2 c) 2.2-5.2 d) all possible