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What is the pH of 15 mL of 0.0045 M HNO3?
pH = - log10 [H+], where [H+] is the molar concentration of hydrogen ions. HNO3 is a strong acid and dissociates completely in water so a 5 M solution of HNO3 would have a concentration of hydrogen ions of 5M also. So, pH = -log10[5] = -0.699 which indicates an extremely strong acid.
What is the concentration of HNO3 in a solution with pH3.4?
1/103.4= 4.0 x 10 -4 M HNO3==============
How many milliliters of a stock solution of 11.1 m hno3 would be needed to prepare 0.500 l of 0.500 m hno3?
Use the equation; MaVa= MbVbWhere M is Molarity and V is volume.For this question, the left side of the equation is the information for 0.12M HNO3The unknown will be x on the right of the equation (replace Vb with x and solve for x).After the answer is found, it will need to be converted to mL, 1 L=1000mL
How many milliliters of a stock solution of 11.4 m hno3 would you have to use to prepare 0.500 l of 0.470 m hno3?
500 x .50/1000 x 1/1 x 1000/6.0 = 41.7 = 42 mL HNO3
A 3.0-milliliter sample of hno3 solution is exactly neutralized by 6.0 milliliters of 0.50 m koh what is the molarity of the hno3 sample?
1.0 Moles
How many moles of hno3 are needed to prepare 5.0 of a 2.0 m solution of hno3?
10
What is the pH of 15 mL of 0.0045 M HNO3?
pH = - log10 [H+], where [H+] is the molar concentration of hydrogen ions. HNO3 is a strong acid and dissociates completely in water so a 5 M solution of HNO3 would have a concentration of hydrogen ions of 5M also. So, pH = -log10[5] = -0.699 which indicates an extremely strong acid.
What is the concentration of HNO3 in a solution with pH3.4?
1/103.4= 4.0 x 10 -4 M HNO3==============
How many milliliters of a stock solution of 11.1 m hno3 would be needed to prepare 0.500 l of 0.500 m hno3?
Use the equation; MaVa= MbVbWhere M is Molarity and V is volume.For this question, the left side of the equation is the information for 0.12M HNO3The unknown will be x on the right of the equation (replace Vb with x and solve for x).After the answer is found, it will need to be converted to mL, 1 L=1000mL
What is the mean average of 6 15 and m?
The average of 6, 15 and m is (6 + 15 + m) / 3 = (21 + m)/3 = 7 + m/3
How many milliliters of a stock solution of 11.4 m hno3 would you have to use to prepare 0.500 l of 0.470 m hno3?
500 x .50/1000 x 1/1 x 1000/6.0 = 41.7 = 42 mL HNO3
What is the molarity of a solution dissolve 0.31 grams of HNO3 in 300ml of water?
Molarity = moles of solute/Liters of solution ( get moles of HNO3 and 300 ml = 0.300 Liters ) 0.31 grams Nitric acid (1 mole HNO3/63.018 grams) = 0.004919 moles HNO3 Molarity = 0.004919 moles HNO3/0.300 Liters = 0.0164 M HNO3
A 3.0-milliliter sample of hno3 solution is exactly neutralized by 6.0 milliliters of 0.50 m koh what is the molarity of the hno3 sample?
1.0 Moles
What is the molarity of an naoh solution if 4.37ml is titrated by 11.1 ml of 0.0904 m hno3?
0.289 Moles is the molarity of an NaOH solution if 4.37 ml is titrated by 11.1 ml of 0.0904m hno3.
What does 15 F of M mean?
if the question were 15 M of F then answer is 15 Minutes of Fame which was a quote from Andy Warhol
What does m2 - 8m 15 equal?
If you mean m^2 -8m +15 then it equals (m -3)(m -5) when factored
What is the molarity of OH- in an aqueous solution that is 0.34 M HNO3?
1.00 * 10^-14/ 0.34 = 2.9^-14 M or (3.2e-14 M)
