Question
hello!!!
what volume of hydrochloric acid concentration 0.1 mol is required to neutralise 100 cm3 of sodium hydroxide solution concentration 0.1 mol
can you please expalin this question step by step i really don't understandand how to do it thank you very much
what volume of hydrochloric acid concentration 0.1 mol is required to neutralise 100 cm3 of sodium hydroxide solution concentration 0.1 mol
can you please expalin this question step by step i really don't understandand how to do it thank you very much
Answers
DrBob222
Step 1. Write and balance the equation.
HCl + NaOH ==> NaCl + H2O
Step 2.
How many mols NaOH do you have to neutralize?
M x L = mols = 0.1 M x 0.100 L = 0.01 mol NaOH.
Step 3.
Convert mols NaOH to mols HCl using the coefficients in the balanced quation.
0.01 mol NaOH x (1 mol HCl/1 mol NaOH) = 0.01 mol HCl needed.
Step 4.
M HCl = mols HCl/L HCl.
You have M HCl, you have mols HCl, calculate L HCl. I think the answer is 0.1 L or 100 cc of O.1 M HCl but check me out on that.
HCl + NaOH ==> NaCl + H2O
Step 2.
How many mols NaOH do you have to neutralize?
M x L = mols = 0.1 M x 0.100 L = 0.01 mol NaOH.
Step 3.
Convert mols NaOH to mols HCl using the coefficients in the balanced quation.
0.01 mol NaOH x (1 mol HCl/1 mol NaOH) = 0.01 mol HCl needed.
Step 4.
M HCl = mols HCl/L HCl.
You have M HCl, you have mols HCl, calculate L HCl. I think the answer is 0.1 L or 100 cc of O.1 M HCl but check me out on that.