Concentrated H 2SO 4 (MW = 98.08 g/mol) is 18.0 M and has a density of 1.84 g/mL. What is the percent concentration of acid if 10.0 mL of the concentrated acid is added to 25.0 mL of water?

6. What is the molarity of a 3.25m CaCl solution? (density = 1.02 g/mL)?

If 24.5 mL of a 0.145 M NaOH solution are needed to neutralize 0.520 g of an unknown monoprotic acid, what is the molar mass of the acid?

How many moles of H+ ions are present in 456 mL of 0.943 M nitric acid solution? mol Ht

If 50.0g of CH3OH (MM = 32.04 g/mol) are dissolved in 500.0 mL of solution, what is the concentration of CH3OH in the solution?

If 2.00 grams of an unknown DIPROTIC acid (H2A) is titrated with 34.0 mL of 1.35 M NaOH, what is the molar mass (g/mol) of the diprotic acid? H2A+2NaOH⟶2H2O+Na2AH2A+2NaOH⟶2H2O+Na2A (Hint: See equation below in which mm is molar mass (units: g/mol), m is mass (unit: g), and mol isnumber of moles (unit: mol)). mmacid=macidmolacidmmacid=macidmolacid Molar Mass =  ___________   g/mol (input the numeric value only!) Remember: use correct significant figure rules. Significant figures always matter in Chemistry!

If 18.3 g of CH₃OH (MM = 32.04 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of CH₃OH in the resulting solution?

if you tritate 10.00 mL of vinegar with .310 M NaOH and determine that the end point is reached after the addition of 15.21 mL of NaOH, calculate the molarity of the acid in the vinegar.

What is the concentration of HNO3 in the final solution when 70.0 mL of a 6.00 M HNO3 solution is diluted with pure water to a total volume of 0.15L ?

You need to prepare 1.0 L of 2.0 M H2SO4.  In the store room is a bottle of 18.0 M  H2SO4.  What volume of concentrated acid do you need to measure out and what volume of water do you need to add to prepare your solution?