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i need help with finding the ph of an aq solution. im confused 9,10,12,13,14, &15. on...
A buffer solution contains 1.0 M HF and 1.0 M NaF. The ka for HF is 7.2x10-5. 0.10 moles of HCl are added to 1 liter of the buffer. The pH of the resulting solution is a) 4.05 b) 4.14 c) 4.23 d) 4.74
i already know they answer please explain your solutions Ka for CH3COOH = 1.8x10^-5 pka i calculated 4.74 ID: A fer- a solut monione blir rw Name: was 11. If 0.40 g of solid NaOH is added to 1.0 liter of a buffer solution that is 0.10 Min CH,COOH and 0.10 Min NaCH,COO, how will the pH of the solution change? a. The pH increases from 4.74 to 4.83. b. The pH decreases from 7.00 to 4.83. c. The pH...
5. A) What is the pH of 2.5 M CH3COOH aqueous solution? Ka of CH3COOH at 25°C is 1.8x 10-5? - B) What is the pH of 1 M NHz aqueous solution? Kb of NH3 at 25°C is 1.8x 10-5?
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...
what is the ph of a buffer that contains 0.15 m ch3cooh and 0.10 m nach3coo (ka=1.8x10-5)? a. 4.74 b. 7.00 c. 4.57 d.4.92
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...
Calculate the pH of the following solution (Ka HCO2H is 1.8x10-4 and Kb NH3 is 1.8x10-5): 0.10 M HCO2H / 0.10M NaHCO2 buffer
5. You need to make 500.0 mL of a buffer with a pH of 2.20. You have the following substances to work with: 0.100 M NH3 Solid NaN3 Solid NaClO2 0.100 M HClO2 Solid NH4Cl Solid Na2SO3 0.100 M HN3 Solid NaHSO3 Ka for HClO2 = 1.1x10-2 Kb for NH3 = 1.8x10-5 Ka for HN3 = 1.9x10-5 Ka1 for H2SO3 = 1.7x10-2 Ka2 for H2SO3 = 6.4x10-8 (Assume that the addition of solid does not change the volume of the...
1. Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.350 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10-5 (a) 5.137 (b) 4.367 (c) 9.633 (d) 8.781 (e) 8.863 2. A 0.1 M solution of which of the following willl have the highest pH? (a) KCN, Ka of HCN = 4.0x10-10 (b) NH4NO3, Kb of NH3 = 1.8x10-5 (c) NaOAc, Ka of HOAc...
Additional Aspects of aqueous balances: 2. Determine the pH of a buffer solution consisting of 0.50M of CH3COOH and 0.50M of CH3COO- . Ka=1.8x10^-5