Question

Is the molarity of a solution that contains 6 moles of solute in 2 liters of solution 12 M????

Answer 1

Okay. I'll try to help.
Molarity is concentration of a solution expressed as the following:

#moles solute (or dissolved stuff)/1 L solution

So a 1M solution would be a solution where in 1 liter, there is one mole of solute.

But no. The molarity of a solution with 6 moles of solute in 2 liters is:

6 moles/2 L=3M.
But I think you accidentally multiplied instead of dividing. I hope this helps.

Answer 2

thankyou

Answer 3

U2 L10 Unit Test
Connexus Academy

1. What is the maximum amount of KCI that can dissolve in 200 g of water? (The solubility of KCI is 34 g/100 g H2O at 20°C)
C, 68 g

2. For most solids, which of the following occurs as temperature increases?
B, Solubility increases.

3. If the solubility of a gas in water is 4.0 g/L when the pressure of the gas above the water is 3.0 atm, what is the pressure of the gas above the water when the solubility of the gas is 1.0 g/L?
D, 3 M

4. What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?
A, 6 M

5. What mass of Na2SO4 is needed to make 2.5 L of 2.0 M solution? (Na = 23 g; S = 32 g; O = 16 g)
D, 710 g

6. The volume of 6.00M HCI needed to make 319 mL of 6.80M HCI is ____.
D, 362 mL

7. If the percent (mass/mass) for a solute if 4% an the mass of the solution is 200 g, what is the mass of solute in solution?
A, 8.0 g

8. Colligative properties depend upon the ____.
C, number of solute particles in a solution

9. What is the formula for phosphoric acid?
B, H3PO4

10. Which of these is an Arrhenius base?
A, LiOH

11. A Lewis acid is a substance that can ____.
B, accept a pair of electrons

12. Which compound can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base?
A, water

13. What are the acids in the following equilibrium reaction?
CN- + H2O = HCN + OH-
B, H20, HCN

14. The products of self-ionization of water are____.
D, OH- and H+

15. Which type of solution is one with a pH of 8?
B, basic

16. The acid dissociation constant for an acid dissolved in water is equal to the ____.
B, equilibrium constant times the concentration of water

17. A 0.12 M solution of an acid that ionizes only slightly in solution would be termed ____.
C, dilute and weak

18. If the solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the solubility of the gas when the pressure is 202 kPa? Show your work.
*Short answer question, you have to answer this yourself sorry!*

19. Explain on a particle basis how the addition of a solute affects the boiling point, the freezing point, and the vapor pressure of the solvent.
*Short answer question, you have to do this yourself sorry!*

20. Calculate the hydrogen-ion concentration [H+] for the aqueous solution in which [OH] is 1 x 10^-11 mol/L. Is this solution acidic, basic, or neutral? Show your work.
*Short answer question, you have to do this yourself sorry!*

21. Calculate the acid dissociation of a weak monoprotic acid if a 0.5 solution of this acid gives a hydrogen-ion concentration of 0.001 m? Show your work. Hint: monoprotic means containing one proton.
*Short answer question, you have to do this yourself sorry!*

22. Compare and contrast the properties of acids and bases. Include two similarities and two differences.
*Short answer question, you have to do this yourself sorry!*

Answer 4

Thank you so much omg