Caculate the PH THANK YOU!
[OH−] = 1.9×10−7 M
[OH−] = 1.6×10−8 M
[OH−] = 7.2×10−11
[OH−] = 7.2×10−2 M
9.28×10−3 M KOH
7.89×10−3 M HNO3
5.54×10−4 M Sr(OH)2
Caculate the PH THANK YOU! [OH−] = 1.9×10−7 M [OH−] = 1.6×10−8 M [OH−] = 7.2×10−11...
Calculate the pH of each solution. A. 7.55×10−2 M HBr B. 6.28×10−3 M KOH C. 1.89×10−3 M HNO3 D. 5.54×10−4 M Sr(OH)2 E. [OH−] = 9.9×10−7 M F. [OH−] = 8.6×10−8 M G. [OH−] = 9.2×10−11 M H. [OH−] = 3.4×10−2 M
Calculate the PH 1.) 9.55×10−2 M HBr 2.) 1.28×10−3 M KOH 3.) 8.89×10−3 M HNO3 4.) 2.54×10−4 M Sr(OH)2
Calculate [OH -] and pH for each of the following solutions. (a) 0.0061 M KOH [OH-] = ? M pH=? (b) 0.0225 g of KOH in 540.0 mL of solution [OH-] = ? M pH=? (c) 53.0 mL of 0.00788 M Sr(OH)2 diluted to 700 mL [OH-] = ? M pH=? (d) A solution formed by mixing 44.0 mL of 0.000590 M Sr(OH)2 with 25.0 mL of 3.2 x 10-3 M KOH [OH-] = ? M pH=? Calculate [OH-] and...
For each of the following strong base solutions, determine [OH−],[H3O+], pH, and pOH. A) 1.6×10−3 M Ca(OH)2 Express your answer using two significant figures. (OH-), (H3O+) Enter your answers numerically separated by commas. pH, pOH. Express your answer to two decimal places. Enter your answers numerically separated by commas. B) 4.9×10−4 M Sr(OH)2 Express your answer using two significant figures. Enter your answers numerically separated by commas: pH, pOH. Express your answer to two decimal places. Enter your answers numerically...
Calculate the pH of each solution. [OH−] = 9.9×10−7 M [OH−] = 6.6×10−8 M [OH−] = 5.2×10−11 M [OH−] = 9.5×10−2 M pOH = 2.7
Question 9 of 12 Submit What is the pH of a 9.7 x 10-6 M KOH solution? 1 4 7 +/- 2 5 8 : 3 6 9 0 x 10 Question 10 of 12 Submit The pOH of 0.0240 M solution of Sr(OH)2 is 1 4 7 +/- 2 5 8 : 3 6 9 0 x 10
26. + -10.1 points 0/4 Submissions Used Calculate [OH-] and pH for each of the following solutions. (a) 0.0054 M CSOH [OH-] = M pH = (b) 0.0136 g of KOH in 530.0 mL of solution [OH-] = M pH = (C) 15.2 mL of 0.00283 M Sr(OH)2 diluted to 1000 mL [OH-] = M pH = (d) A solution formed by mixing 81.0 mL of 0.000470 M Sr(OH)2 with 38.0 mL of 5.6 x 10-3 M CSOH [OH-] =...
show work when solving the table please, thank you pH of pure water 7,00 130* 10/10-"M(OH) .0X10-”M KW 1.0210-14 Initial Burette Reading 0.00 mL (KOH) 6,100M pH KOH Additions [H30+] * [OH-] + Kw Min = M2 V 2 5.01010-12 1.96810 3 9.427x65 6.1M) (1) = m2 (51) 12.51*10-12 3.85X10319.66176-15 11.86x10-12 19927710 vs bo 101190 Burette Reading 1.00 mL [ 11.30 2.0 mL 11.60 3.00mL 1173 4.00 mL 5.00 ml 11.98 6.00 mL 7.00 ml 4.00 ml 12.15 9.10mLL 12.11...
What is the pH of a solution that has a hydroxide concentration of 1.9 X 10-5 M? What is the pH of a 0.056 M solution of H2SO4? H2SO4 is a strong acid. Calculate the pH of a 0.50 M solution of Sr(OH)2. Sr(OH)2 is a strong base. Mylanta liquid has 200 mg of Al(OH)3 and 200 mg of Mg(OH)2 per teaspoonful. Write the equation for the neutralization of stomach acid. Assuming both bases are completely soluble in water, calculate...
Calculate pH part a) [OH-] = 8.9 x 10^-7 M part b) [OH-] = 7.6 x 10^-8 M part c) [OH-] = 6.2 x 10^-11 M part d) [OH-] = 1.5 x 10^-2 M