1a. Calculate the pH of a 8.01 × 10−5M HBr solution.
Report your answer to TWO places past the decimal.
1b. . Calculate the pH of a 1.39 × 10−6M HNO3 solution.
Report your answer to TWO places past the decimal.
1c. Calculate the pH of a 0.00963 M Ca(OH)2 solution.
Report your answer to TWO places past the decimal.
1d. Calculate the pH of a 0.00155 M Ca(OH)2 solution.
Report your answer to TWO places past the decimal.
1e. Calculate the pH of a solution that contains 0.0705 g of Ba(OH)2 in 1.65 L of water.
Report your answer to TWO places past the decimal.
1f. Calculate the pH of a solution that contains 0.0243 g of Mg(OH)2 in 2.11 L of water.
Report your answer to TWO places past the decimal.
please answer all parts and show your work thank you so much!!
(1a): HBr is strong acid , it will dissociate completely in the solution . [HBr] = [H+] = 8.01×10-5M
pH = - log[H+] = 5 - log(8.01) = 4.096 = 4.10 (answer)
(1b) : concentration of HNO3 is very small, we need to consider the concentration from water also.
[H+] = (1.39×10-6 + 10-7 )M = 1.49×10-6
pH = - log(1.49×10-6) = 5.827 = 5.83 (answer)
(1c) : Concentration of Ca (OH)2 = 0.00963M ,
Concentration of OH- = 2 × 0.00963M = 0.01926M
pOH = - log(0.01926) = 1.7153
pH = 14 - pOH = 14 - 1.7153 = 12.2847 = 12.18 (answer)
(1d) : [OH-] = 2 × 0.00155M = 0.00310
pOH = - log(0.00310) = 2.5086
pH = 14 - pOH = 14 - 2.5086 = 11.4914 = 11.49 (answer)
(1e) : molarity = (mass of substance /molar mass )/volume of solution(L)
molarity of Ba(OH)2 = (0.0705g / 171.342g/mol)/1.65L = 2.4937×10-4M
[OH-] = 2×2.4937×10-4M
pOH = 3.302
pH = 14 - pOH = 14 - 3.302 = 10.698 = 10.70 (answer)
1a. Calculate the pH of a 8.01 × 10−5M HBr solution. Report your answer to TWO places past the de...
1a. Calculate the pH of a 1.35 × 10−4M HNO3 solution. Report your answer to TWO places past the decimal. 1b. Calculate the pH of a 3.25 × 10−6M HClO3 solution. Report your answer to TWO places past the decimal. 1c Calculate the pH of a 0.00852 M RbOH solution. Report your answer to TWO places past the decimal. 1d. Calculate the pH of a solution that contains 0.0727 g of Ca(OH)2 in 1.83 L of water. Report your answer...
1f. Calculate the pH of a solution that contains 0.0243 g of Mg(OH)2 in 2.11 L of water. Report your answer to TWO places past the decimal. thanks so much! please show work!
1a. Calculate the pH of a 3.95 × 10−3M HNO3 solution. Report your answer to TWO places past the decimal. 1b. Calculate the pH of a 4.64 × 10−6M HI solution. Report your answer to TWO places past the decimal. 1c. Calculate the pH of a 0.00312 M RbOH solution. Report your answer to TWO places past the decimal. 1d. Calculate the pH of a 0.006 M RbOH solution. Report your answer to TWO places past the decimal.
1a. Calculate the pH of a solution that contains 0.0282 g of NaOH in 1.50 L of water. Report your answer to TWO places past the decimal. 1b. Calculate the pH of a solution that contains 0.0261 g of Ba(OH)2 in 2.04 L of water. Report your answer to TWO places past the decimal.
Calculate the pH of a solution that contains 0.0623 g of RbOH in 1.88 L of water. Report your answer to TWO places past the decimal.
Calculate the pH of a 0.400 M HNO2 solution. Report answer to 2 decimal places. Ka = 7.1 x 10-4 HNO2 (aq) + H20 (1) = NO2 (aq) + H30+ (aq) Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200 M CH3NH3 (methylammonium chlorides Report answer to 2 decimal places. CHH) - 4.4 x 10-4 CH3NH2 (aq) + H200 - Chynas (aq) + OH" () 1. Questa
Calculate the pH of a 5.2 x 10-8 M HCl solution. Report your answer to the hundredths place. < Feedback pH = 6.61 Because the concentration of the HCl solution is so small, you must account fot the autoionization of water when calculating the pH. What fraction of the total H+ in this solution is from the HCI? Report your answer to the hundredths p Start with the charge balance equation for this solution. fraction: 0.21 [H+] = [OH-] +...
Question 7 (2 points) Calculate the pH of 0.0020 M Ca(OH)2 solution. Provide your answer to two places after the decimal. Your Answer: Answer
Question 15 (2 points) Calculate the pH of 0.0030 M Ca(OH)2 solution. Provide your answer to two places after the decimal. Your Answer: Answer
Calculate the pH of 0.34 M ZnCl2 solution. Express your answer using two decimal places.