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Calculate the pH of a solution that is 0.50 M in HF (Ka = 7.2 x10-4) and1.50 M in NaF. A. 10.56 B. 3.62 C. 3.44 D. 0.30 E. 3.14
Find the pH and percent ionization for each HF solution. (Ka for HF is 6.8 x10-4.) Please use this Ka that is given to solve a. 0.250 M HF b. 0.100 M HF c. 0.050 M HF
Kw 1.0 x 1014 Ks 6.6 X 10 for HF Kb 1.8 X 10 for NH 1. Calculate the [H'], [OHl, pH and pOH for 0.025 M HCl 2. Calculate the pH of 4.0 M hydrofluoric acid, HF. (over)
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...
calculate the pH and % ionization of 0.0200 M HF (Ka=6.8x10^-4)
Calculate the pH of a buffer that is 0.040 M HF and 0.020 M LIF. The Ka for HF is 3.5 x 10-4.
8) The Ka of hydrofluoric acid (HF) at 25.0 C is 6.8 x10-4. What is the pH of a 0.15 M aqueous 8) solution of HF? A) 4.60 B) 0.82 C)3.64 D) 1.17 E) 2.00
1. Calculate the pH of a solution that is 1.00 M HF, 1.00 M HCl, and 1.439 MNaF. (Ka= 7.2 x10–4) 3.14 3.30 2.48 2.98 0.25 I am getting 2.48 for this one 2. Calculate the pH of a solution that is 1.00 MHF, 2.00 M HCl, and 1.439 MNaF. (Ka= 7.2 x10–4) 3.14 3.30 2.48 2.98 0.25 and for the second one i keep getting 2.48 or 0.25. Which one is it??
4. Calculate [H30*], [OH-], pH and pOH of a 0.5 M CH3COOH solution, Ka = 1.8 x 10-5.
Calculate the following values for a 0.025 M solution of Hydrocyanic acid. Ka= 4.90 × 10^-10 [H3O+]eq [OH-]eq = pH = pOH = % Ionization =