please help me please i dont have questions remaining anymore
please help me please i dont have questions remaining anymore A solution is prepared by dissolving 0.060 mol of iodoacet...
A solution is prepared by dissolving 0.075 mol of cyanoacetic acid (Ka-3.37×10-3) and 0.030 mol of sodium cyanoacetate in water to a total solution volume of 1.00 L. First, calculate a pH for the solution by assuming that the concentrations of NCCH2CO2H and NCCH2CO2 are equal to the formal concentrations of the substances dissolved. 2.07 Computer's answer now shown above. You are correct. Your receipt no. is 160-8794 () Previous Tries Next, calculate the pH for the solution based on...
A solution is prepared by dissolving 0.045 mol of 4-nitrobenzoic acid (Ka = 3.61×10-4) and 0.030 mol of sodium 4-nitrobenzoate in water to a total solution volume of 1.00 L.First, calculate a pH for the solution by assuming that the concentrations of 4−(NO2)C6H4CO2H and 4−(NO2)C6H4CO2− are equal to the formal concentrations of the substances dissolved. Next, calculate the pH for the solution based on the equilibrium concentrations of 4−(NO2)C6H4CO2H and 4−(NO2)C6H4CO2−. Use the Henderson-Hasselbalch approximation to calculate the pH of...
24. (25 points) A buffer solution was prepared by dissolving 0.500 mol formic acid and 0.060 mol sodium formate in enough water to make 1 L of solution, K, for formic acid is 1.80 x 104 a) Calculate the pH of the solution. b) If this solution was diluted to 10 times its volume, what would be the pH.
i need help with 6 b) please 6. a) Calculate the pH of a solution prepared by dissolving 0.0775 mol acetic acid and 0.0460 mol sodium acetate in 1 L of water. (Ka = 1.8 x 10-5) ANSWER: 4.52 b) Calculate the pH of the above solution if 0.0100 mol of KOH is added to this solution. ANSWER: 4.66
QUESTION 14 Calculate the pH of a solution prepared by dissolving 0.270 mol of formic acid (HCO2H) and 0.230 mol of sodium formate (NaCO2H) in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77X104 Enter your answer with three decimal places.
Calculate the pH of a solution prepared by dissolving 0.050 mol of benzoic acid (HA) and 0.50 mol of sodium benzoate (A-) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.30 x 10-5 A. 5.20 B. 1.30 C. 7.00 D. 3.20 E. 4.20
what is the ph of a solution prepared by dissolving 0.50 mol of acetic acid and 0.2 mol of sodium acetate in water and adjusting the volume of 0.5L if the pka for acetic acid is 4.75. of 0.010 mol of sodium hydroxide is added to the buffer solution from part (a), determine the ph of the new solution
Calculate the pH of a buffer solution prepared by dissolving 19.50 g of sodium cyanate NaCNO (65.01g/mol) in 1.00 M cyanic acid (HCNO) to a final volume of 1.00 liter of solution. Ka(HCNO) = 3.50 x 10-4
Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid HCOOH and 0.230 mol of sodium formate HCOONa in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77x10. -4 Seleccione una: a. 10.463 b. 2.307 O O c. 2.099 d. 3.546 e. 3.952
A buffer solution was prepared by adding 4.72 g of sodium acetate, NaCH, CO2, to 2.50 10 mL of 0.100 M acetic acid, CH3CO,H (K, = 1.8 x 10-6). a What is the pH of the buffer? pH = 5.10 Correct Find the pH using the Henderson-Hasselbalch equation: 4.72 g 1 mol NaCH, CO2 CH,CO2- ] = [NaCH,CO2] = 0.250 L -= 0.230 M 82.03 g [CH, CO2- pH = pK,+ logo = -log(1.8 x 10-5) + log CH, CO2H]...