10.0 g of the strong base, KOH, is dissolved in 2000 mL of solution. What is...

Question

Question

10.0 g of the strong base, KOH, is dissolved in 20

Answer 1

Answer #1

molarity = mass of solute *1000/gram molar mass of solute * volume of solution in ml

= 10*1000/56*2000 = 0.089M

KOH is strong base

KOH -------> K⁺ + OH^-

0.089M 0.089M

[OH-] = [KOH]

[OH-] = 0.089M

POH = -log[OH-]

= -log0.089

= 1.0506

PH = 14-POH

= 14-1.0506 = 13

a. 13 >>>> answer

Answer 2

Similar Homework Help Questions

Calculate [OH−] for this strong base solution: 1.085 g of KOH in 410.0 mL of solution....

Calculate [OH−] for this strong base solution: 1.085 g of KOH in 410.0 mL of solution. Calculate [OH−] for this strong base solution: 14.0 mL of 1.50×10−2 M Ca(OH)2 diluted to 460.0 mL. Calculate [OH−] for the strong base solution formed by mixing 14.0 mL of 1.00×10−2 M Ba(OH)2 with 33.0 mL of 7.6×10−3 M NaOH.
Calculate [OH−] for this strong base solution: 1.085 g of KOH in 410.0 mL of solution....

Calculate [OH−] for this strong base solution: 1.085 g of KOH in 410.0 mL of solution. Calculate [OH−] for this strong base solution: 14.0 mL of 1.50×10−2 M Ca(OH)2 diluted to 460.0 mL. Calculate [OH−] for the strong base solution formed by mixing 14.0 mL of 1.00×10−2 M Ba(OH)2 with 33.0 mL of 7.6×10−3 M NaOH.
11.5 g of KOH (s) is dissolved up to 250.0 mL in water. What is the...

11.5 g of KOH (s) is dissolved up to 250.0 mL in water. What is the molarity of this solution? Molarity of first solution: Enter your answer here M KOH If we then add an additional 2.750 L of water to the solution what is the new molarity? Molarity of second solution: Enter your answer here M KOH For this second solution calculate the pH, pOH and [H3O+). pH = Enter your answer here pOH = Enter your answer here...

Titration of a diprotic acid with a strong base You have a 10.0 mL solution containing...

Titration of a diprotic acid with a strong base You have a 10.0 mL solution containing 0.5 M carbonic acid. Carbonic acid is diprotic, with pKa1 = 6.35 and pKa2 = 10.33. You titrate this solution using 1.00 M NaOH . (a) Calculate the pH of the solution before adding any NaOH. (b) Calculate the amount of NaOH needed to reach the first midpoint. What is the pH? (c) Calculate the amount of NaOH needed to reach the first equivalence...
17) What is the pH of an aqueous 0.305 M KOH solution (a strong base)? TO...

17) What is the pH of an aqueous 0.305 M KOH solution (a strong base)? TO 18) What is the [OH-] of a bleach sample that registers 11.41 on a pH meter? -8-
4. What is the molarity of a solution containing 10.0 g AgNO3 dissolved in 500. ml...

4. What is the molarity of a solution containing 10.0 g AgNO3 dissolved in 500. ml of solution?

2. calculate the concentration of the following solution. 126.9 g of KOH dissolved in 263.6 mL...

2. calculate the concentration of the following solution. 126.9 g of KOH dissolved in 263.6 mL
please help!! thank you 11.5 g of KOH (s) is dissolved up to 250.0 mL in...

please help!! thank you 11.5 g of KOH (s) is dissolved up to 250.0 mL in water. What is the molarity of this solution? Molarity of first solution: Enter your answer here M KOH If we then add an additional 2.750 L of water to the solution what is the new molarity? Molarity of second solution: Enter your answer here M KOH For this second solution calculate the pH, pOH and [H3O+). pH = Enter your answer here pOH =...
10.0 g of acetic acid (CH,COOH) is dissolved in a 500.0 ml solution. What is the...

10.0 g of acetic acid (CH,COOH) is dissolved in a 500.0 ml solution. What is the molarity? Report your answer with the correct number of significant figures. Provide your answer below: M

what is the ph of the following solutions? 150 g NH4CI dissolved into 10.0 mL of...

what is the ph of the following solutions? 150 g NH4CI dissolved into 10.0 mL of a 0.100 M NaOH. Assume a fine! volume of 10.1 mL. NH3 kb= 1.8x10^5