Questions LLC
Login
or
Sign Up
Ask a New Question
Chemistry
Chemical Reactions
Acid-base reactions
45.00 mL of 1.45×10−2 M HI(aq) is mixed with 75.00 mL of 1.06×10−2 M KOH(aq).
1 answer
Sorry, I forgot to mention what the actual question was using the information I just posted.
What is the pH of the final solution?
You can
ask a new question
or
answer this question
.
Related Questions
How many grams of solute are contained in 64.3 mL of 0.0238M KOH?
Do I convert 64.3ml to L=.0643L Multiiply .0643L and .0238M
Suppose that 30.0 mL of 0.20 M C6H5COOH(aq) is titrated with 0.30 M KOH(aq).
(a) What is the initial pH of the 0.20 M
IF 8.5g of KOH powder are placed in 100g of water at room temperature of 20degree Celsius, what is the final temperature of the
Please help me figure out where I went wrong.
HNO3 + KOH -> KNO3 + H2O enthalpy change = -53.4 kJ/mol 55.0 mL of 1.30 mol/L
Calculate the molarity of the following solutions:
5.0g of KOH in 4.0L of KOH solution I went from grams of KOH to moles of KOH
If we combined 18.00 g of KOH and 18.00 g of H2SO4 , and they reacted according to the equation below, how many moles of K2SO4
A solution of KOH is prepared by dissolving 2.00 g of KOH in water to a final volume of 250 ml of solution what volume of this
Suppose that 30.0 mL of 0.20 M C6H5COOH(aq) is titrated with 0.30 M KOH(aq)
(a) What is the initial pH of the 0.20 M
A solution of 10.m koh was used to prepare 2.00L of 0.500 M KoH how many millilitres of the original KOH solution are needed
if 22.5 mL of 0.383 M HCl are required to completely neutralize 20.0 mL of KOH, what is the molarity of the KOH solution?
