What is the pH of a 0.4 M sodium carbonate solution? Carbonate has a Kb of 2.1 x 10-4.
What is the pH of a 0.4 M sodium carbonate solution? Carbonate has a Kb of...
1. What is the pH of a buffer solution prepared with a 0.4 M sodium citrate and 1% citric acid (pka for citric acid - 3.13, MW - 192 g/mol)? 8. A buffer solution is prepared using 0.4 mole of a weakly basic drug (pka - 10.1) and an unknown quantity of its salt. The final solution has a pH of 8.99. How much of the salt was used? 9. A buffer solution with a desired pH of 8.15 needs...
Describe how to make 2.0L of a 2.00 M solution of sodium carbonate from solid sodium carbonate(s). b. Describe how you can make a buffer with sodium carbonate(s) by adding hydrochloric acid. c. How many mL of 1.00 M HCl(aq) are needed to be added to 10.00 g of sodium carbonate to make a buffer at pH =10.00. Ka of HCO3- is 4.7 x 10-11.
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
Calculate the pH of a 0.445 M NH, solution. NH, has a Kb = 1.8 x 10-5. pH = The K, of a weak monoprotic acid is 1.59 x 10-5. What is the pH of a 0.0808 M solution of this acid? pH =
QUESTION 10 What is the pH of a 0.30 M pyridine solution that has a Kb = 1.9 x 10-97 The equation for the dissociation of pyridine is CsH5N(aq) + H2O(1 =C5H5NH+ (aq) + OH" (aq). Kw = 1.0 x 10-14 10.38 4.62 9.38 8.72
What is the Kb of X1- if a 0.0220-M solution of KX has a pH of 12.007? Kb
What is the pH of a 0.35 M A solution that has a Kb-3.7 x 10-6 ? The equation for the dissociation of A is: A (aq) + H20 (99) =HA (aq) + OH(aq) Answer to two decimal places.
1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown weak base is 4.7 x 10−6. 2) An unknown weak acid solution with a concentration of 0.0850 M has a pH of 4.35. What is the Ka for this weak acid? 3) What is the pH of a 0.0380 M solution of HNO2? (Use your workbook to find Ka) 4) An unknown weak base solution with a concentration of 0.187 M has a pH...
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
What is the pH of a 0.200 M CH3NH2 solution? (Kb for CH3NH2 = 4.4 x 10-4) 2.03 11.97 9.33 8.79