QUESTION 4 Calculate the pH when 1.13 g of NaClO (FW = 74.44 g/mol) is added...
Calculate the pH when 1.03 g of CH3COONa (FW = 82.03 g/mol) is added to 36 mL of 0.500 M acetic acid, CH3COOH. Ignore any changes in volume. The Ka value for CH3COOH is 1.8 x 10-5.
Calculate the pH when 1.61 g of CH3COONa (FW = 82.03 g/mol) is added to 34 mL of 0.500 M acetic acid, CH3COOH. Ignore any changes in volume. The Ka value for CH3COOH is 1.8 x 10-5.
The pH of 0.50 M HClO is 3.91. Calculate the change in pH when 1.29 g of NaClO is added to 18 mL of 0.50 M HClO. Ignore any changes in volume. The Ka value for HClO is 3.0 x 10-8.
QUESTION 9 The pH of 0.50 M acetic acid is 2.52. Calculate the change in pH when 0.91 g of CH3COONa (FW - 82.03 g/mol) is added to 11.1 mL of 0.50 M acetic acid. CH3COOH. Ignore any changes in volume. The Ka value for CH3COOH is 1.8 x 10-5
A buffer solution contains 0.100 mol of HCIO and 0.100 mol of NaClO in 1.00 L. What is the pH of this buffer after 0.010 mol of NaOH are added? HCIO has a Ka = 3.0 x 10-8 07.61 8.47 7.52 O 6.57 7.43
a solution is prepared by mixing 2.50 g of acetic acid (CH3CO2H, FW=60g/mol, Ka=1.75x10^(-5) with 4.70 g of sodium acetate (CH3CO2Na, FW=82g/mol) and adding water to a 500 mL volume. Note that sodium acetate yields Na+ and CH3COO-, the conjugate base of acetic acid. a.) what is the pH? b.) 15mL of 0.50 M HCl were added to the 500 mL solution, what is the pH after addituon of acid? write answer to 3 sig. figured.
A solution was prepared by dissolving 0.200 moles of sodium hypoch lorite (NaClO) in water to a final volume of 1.00 Liter. Ka 2.96x10 for hypochlorous acid (HCIO). Show equations and work steps for these calculations. 1) Calculate Kb of sodium hypochlorite. 2) Calculate the pH of the NaClO solution. 3) Calculate the pH if 10.0 mL of 1.00 M HCl is added to 100.0 mL of the original NACIO solution. 4) Calculate the pH if 20.0 mL of 1.00...
pH of a buffer solution: Mass of NaC2H3O2 * 3H2O (FW=136g/mol): 3.540g Calculate the Theoretical pH of these buffer solutions: A. pH of original buffer solution (with 8.8 mL of 3.0 M acetic acid and 55.6 mL of water) : 4.7 B. pH of buffer + 1.0 mL of 6.0 M HCl: 3.8 C. pH of buffer + 1.0 mL of 6.0 M NaOH: 4.9
a)Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer solution that is prepared by dissolving 4.92g of sodium acetate(molar mass = 82.03gmol^-1) in 250 ml of 0.150 mol L^-1 of acetic acid solution? Assume no change in volume upon addition of either the sodium acetate or HCl. (Ka for acetic acid = 1.8*10^-5) b)Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer...
please explain. thanks
6. A buffer composed of TRIS (FW-121.135 g/mol) and TRIS-HCI (FW-157.596 g/mol, pKa 8.072) contains the following forms in solution: он OH NH," NH +H но Но но но (a) Calculate the pH of a buffer prepared by mixing 13.10 g of TRIS and 9.5 g of TRIS-HCI in 1L of solution. (b) Calculate the pH of the solution in Part (a) after 5 mL of 0.5M NaOH is added