How will you prepare 40% ch3cooh solution?

Q 10 please

How many mL of water should be added to 50.0 mL of a 15.0 M H2SO4 solution to give a final concentration of 0.300 M? A) 950 mL B) 1000 mL C) 2450 mL D) 2500 mL

A potasium carbonate solution is 14.6% KCO3 by mass and has a density of 0.68 g/mL. Calculate molarity of the solution. A. 0.72 M B. 6.67 M C. 12.8 M D. 1.44 M

In a solution the substance which is being disolved is the

Ammonia (NH3, MM 17.031 g/mol) and hypobromite (OBr-) react according to the following chemical reaction. 2 NH3 + 3 OBr- —> N2 + 3Br- + 3 H2O Suppose 0.263 g of ammonia react with 19.0 mL of hypobromite solution. Calculate the concentration of the hypobromite solution

In your first task, you are required to prepare a 100 mL solution of sodium bicarbonate at a concentration of 0.50 M. Complete the following table and calculate the mass of sodium bicarbonate needed to prepare this solution. Molecular weight of sodium bicarbonate Required final concentration Required final volume Amount of sodium bicarbonate needed to make 1 L at 0.5 M Amount of sodium bicarbonate needed to make 100 mL at 0.5 M Mass (g) = Amount (mol) × Molecular Weight (g/mol) Value 84.01 Now that you know the amount of sodium bicarbonate in mol needed to make your solution, you can convert this value into the mass by using the molecular weight of the compound. The following equation may be helpful: Mass of sodium bicarbonate needed to make 100 mL at 0.5 M Units g/mol M (mol/L) L mol mol g In the 100 mL 0.5 M solution, how many molecules of sodium bicarbonate have been added. Hint - In 1 mole there are 6.022 × 10²³ molecules.

A Moving to another question will save this response. Question 13 Which of the following compounds is soluble? O SrCO, O CaCO3 O CuCO, O K,CO3 P Type here to search w F8 F9 F4 F5 F6 F7 F1 F2 F3 # $4 % 3 4

What are the moles of NaOH in each of the 3 trials?

Given chart information attached Calculate the number of moles of acid