What is the pH of a 1.25 L carbonate buffer which was prepared by mixing 0.4098...
Identify the chemical species in the carbonate system, and explain the significance of the system. Hence, on the bases of the following equilibria, determine the concentrations carbonate system species in a stream with a pH of 5.8. CO2(g) ↔ CO2(aq) KH = 3.4 x 10-2 mol L-1 atm-1; CO2(aq) + H2O ↔ H2CO3; Kr = 2 x 10-3 mol L-1 atm-1; H2CO3(aq) ↔ H+ + HCO3-; Ka1 = 4.47 x 10-7 M. HCO3- ↔ H+ + CO32-; Ka2 = 4.68...
1. Calculate the pH of a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5 Calculate the pH of this solution of after the addition of 0.003 L of 0.200 M HCL 2. Consider a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5...
a) Buffer solutions with a pH values of around 10 are prepared using sodium carbonate (Na2CO3) and sodium hydrogen carbonate (NaHCO3). What is the pH of a solution of 10.0g each of the two salts in enough water to make 0.250 L of solution? pKa2= 10.33 b) By how much does the pH change when 3.5mL of 6.0 M HCl is added? c) By how much does the pH of the solution change when 0.92 g of NaOH is added?
You need a carbonate buffer of pH 10.00 in a study you are performing. How many grams of Na2CO (MW 105.99) do you need to add to 0.750 L of freshly prepared 0.250 M NaHCO, (Ka 4.70 x 10-11) bufffer? a. 0.250 b. none of the above c. 0.221 4.70 x 10.11) buffer? d. 23.5 e. 0.00209
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
CHEM 1151K Make-up HW 3 22. What is the pH of a buffer prepared with 1.0 M HC2H302 and 1.0 M C2H3O2? The Ka for acetic acid, HC2H3O2, is 1.8 × 10-5. HC2H3O2(aq) + H2O(/) CHAD-(aq) + H3O+(aq)
A buffer solution is prepared by dissolving 10.0 g of Na2CO3 and 10.0 g of NaHCO3 in 0.250 L of water. What is the final pH of the solution you prepared? Ka = 4.67 x 10-11 Give a short explanation on how you would bring the pH of the above solution to 10 and confirm this
A buffer with pH = 10.15 is to be prepared by addition solid sodium hydrogen carbonate to 1.00 L of 0.300 M sodium carbonate. What mass is required assuming the volume does not change? For carbonic acid, Ka1 = 4.45 x 10-7 and Ka2 = 5.69 x 10-11
A buffer is prepared by mixing 200.0 mL of 0.1500 M NaOH with 200.0 mL of 0.200 M CH3CO2H in a 1-L volumetric flask and then diluted to volume with distilled deionized water. Calculate the pH of the buffer. Ka = 1.75 x 10-5
What is the pH of a sample of river water in which (HCO3-) = 2.0 x 10-4 M and the concentration of dissolved CO2 in equilibrium with atmospheric CO2 is 1.0 x 10-5 M? Chemical Equation: H2CO3(aq) + H2O(l) = HCO3-(aq) + H3O+(aq) pka = 6.37 Henderson Hasselbach equation: pH=pka+log [base]/[acid] A/