If an aqueous solution is very dilute, will its molality be greater than its molarity, nearly the same as its molarity, or smaller than its molarity?

Molality stays nearly the same as its molarity

Explanation:

Let's make an example of this:

An aqueous solution of 1 mol of NaCl is diluited in a volume of 1L (A).

The same solution is diluited in a volume of 1L, but now we have 0.00001 moles of NaCl (B)

Solution A → Concentrated, [NaCl] = 1 M, 1 m

1L = 1kg

Solution B → Diluted, less concentration, Less molarity and molality.

Now, solution B has a volume of 5L, with 2 moles of solute while A, stays the same.

Molarity A = 1M

Molality A = 1m

Molarity B = 0.4 M

Molality B = 0.4 m

In conclussion, stays nearly the same as its molarity

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

i think its 100.

hope this !