Calculate the approximate pH of an aqueous solution of sodium carbonate Na2CO3 , 0.28 M, at 25°C. (Note: consider one decimal place for the pH answer.)
pKa H2CO3 /HCO3− = 6.35, pKa HCO3- /CO32-= 10.30
Calculate the approximate pH of an aqueous solution of sodium carbonate Na2CO3 , 0.28 M, at...
Calculate the approximate pH of an aqueous solution of ammonium chloride, NH4Cl , 0.03 M, and sodium acetate, CH3COONa, 0.12 M at 25°C. (Note: consider one decimal place for the pH answer.) pKa NH4+/NH3 = 9.24 pKa CH3COOH/CH3COO- = 4.76
Calculate the approximate pH of an aqueous solution of a mixture of CH3COOH, 0.27 M, and CH3COONa, 0.15 M, at 25°C. (Note: consider one decimal place for the pH answer.) pKa = 4.76.
Calculate the approximate pH of an aqueous solution of H2S , 0.05 M, and H3PO4, 0.21 M at 25°C. (Note: consider one decimal place for the pH answer.) pKa H2S/HS- = 7.02, pKa HS-/S2- = 13.99 pKaH3PO4/ H2PO4- =2.15, pKaH2PO4-/HPO42-=7.15, pKa HPO42-/ PO43- =12.38
7. Given a buffer solution of sodium hydrogen carbonate (NaHCO3) and sodium carbonate (Na2CO3). a. Calculate the pH of this buffer solution when 0.100M sodium hydrogen carbonate (NaHCO3) and 0.100M sodium carbonate (Na2CO3). (Ka = 7.94 x 10-7) b. Calculate the new pH value of this buffer solution when 1.00mL of 0.100M NaOH is added to to 100mL of this buffer
1) Consider a 0.040 M solution of carbonic acid. Calculate the pH of this solution as well as the equilibrium concentrations of: [H2CO3], [HCO3-], [H3O+], and [CO32-). H2CO3 + H20 5 HCO3 + H30+ K1 = 4.45 x 10-7 HCO3 + H20 5 CO32- + H30+ K2 = 4.69 x 10-11
1. Write a chemical equation showing why a sodium carbonate solution is basic. Calculate the pH of a 0.10 M sodium carbonate solution, Na2CO3 (aq).
Calculate the pH at 25C of a 0.92 M solution of sodium hypochlorite (NaClO). Note that hypochlorous acid (HClO) is a weak acid with a pKa of 7.50 . Round your answer to 1 decimal place.
In experiment 1 you prepared a solution of sodium carbonate. This means you dissolved solid Na2CO3 in water. Since this ionic compound dissolved in water, you now have only its ions swimming around in the solution. What are the aqueous ions in your solution of sodium carbonate? TTT Arial # 3 (12 # TEE Path: p Words:04 QUESTION 2 In experiment 2, you used a solution of HCI. HCl is a strong acid, which means it is 100% ionized in...
Suppose you slowly add solid sodium carbonate (Na2CO3) to a solution that contains 0.030 M Pb2+ and 0.030 M Ni2+. What is the minimum concentration of CO32– that would cause a precipitate to form? (Assume no volume change; for PbCO3, Ksp = 7.4x10–11, and for NiCO3, Ksp = 1.3x10–7)
Calculate the pH and concentration of species present in a polyprotic acid solution.For a 3.44×10-3 M solution ofH2CO3, calculate both the pH and the CO32- ion concentration.H2CO3 + H2O → H3O+ +HCO3-Ka1 = 4.2×10-7HCO3- + H2O → H3O+ +CO32-Ka2 = 4.8×10-11pH =[CO32-] =