Molarity

posted by .

A 15.7mL sample of HNO3 reacts to neutralize 27.7mL of 0.187M KOH solution. What is the molarity of the HNO3 solution?

HNO3 + KOH ==> KNO3 + HOH

mols KOH = L x M = 0.0277 x 0.187 = ??
mols HNO3 = mols KOH (1 mol reacts with 1 mol).
mols HNO3 = L x M
You have mols HNO3 and L, solve for M.

Check my thinking. Check my arithmetic.

I lost you on this one, I got a little confused on the 3rd step.

mols = L x M
mols KOH = 0.0277L x 0.187M = 0.00518 mols KOH.
The equation is
HNO3 + KOH ==> KNO3 + HOH

The equation shows 1 mol HNO3 reacts with 1 mol KOH; therefore, 0.00518 mols KOH requires 0.00518 mol HNO3.

Then mols HNO3 = L x M
0.00518 mol HNO3 = L x M
0.00518 mol HNO3 = 0.0157 L x M/
Solve for M.
Check to make sure I didn't make a typo.

Thanks for your help but I cant seem to get this one to come out to any of my possible answers. I think I am just getting confused on this one for some reason.

What are the possible answers?

0.165
0.330
0.498
0.298
0.198

0.0277*0.187/0.0157 = 0.32993 which rounds to 3 s.f. as 0.330. I see one like that. Don't you?

I got it finally.

Thank You

How much of each starting material would you use to prepare 2.00 L of each of the following solutions?
0.400 M potassium chromate from solid potassium chromate?

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. CHEMISTRY

    HOW CAN U TELL IF HNO3 +KNO3 IS A BUFFER SOLUTION A buffer solution must contain a weak acid and its conjugate base OR a weak base and its conjugate acid. HNO3 is a strong base and KNO3 is the salt of a strong base (KOH) and a strong …
  2. chemistry

    If it requires 54.7mL of a 0.0765 M HCl solution to complete neutralize 25.0 mL of a KOH solution, what is the molarity of the KOH solution.?
  3. high school chem

    if 150 ml of HNO3 of unknown conceration withmethyl orange indicator present is tritrated with [0.163M]KOH, then the red solution turns yellow after 28.9 ml of the KOH is added. what is the molarity of HNO3 solution.
  4. chemisrty

    Nitric acid,HNO3, is available ata a concentration of 16 M. how much would react with 5.58 g of KOH acording to the following equation?
  5. Chemistry

    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 to molarity but still got the wrong answer... 5.0g KOH X 1 mol KOH/56.108g KOH = 5.0 mol KOH/56.108=0.0891 …
  6. Chemistry

    In the following acid—base neutralization reaction HNO3(aq)+ KOH(aq) ----KNO3(aq) + H2O (I) What is the molarity (M) of an HNO3 solution if 50.0 ml is needed to react with 25.0 ml of 0.150M KOH solution?
  7. Chemistry

    the following acid—base neutralization reaction HNO3 (aq)+ KOH (aq) --KNO3(aq) + H2O (I) What is the molarity (M) of an HNO3 solution if 50.0ml is needed to react with 25.0ml of 0.150M KOH solution?
  8. Chemistry

    Can someone please explain this problem to me step by step pleaseeeeeee?
  9. Chemistry

    A volume of 60.0mL of aqueous potassium hydroxide (KOH ) was titrated against a standard solution of sulfuric acid (H 2 SO 4 ). What was the molarity of the KOH solution if 25.7mL of 1.50 M H 2 SO 4 was needed?
  10. Science

    a flask contain 25 ml of HNO3 solution which requires 30 ml of 0.2 M KOH to complete the reaction. calculate the concentration of KOH. HNO3+ KOH= H2O + KNO3

More Similar Questions