Consider the equilibrium

b(aq)+h2o(l) ⇌hb+(aq)+oh−(aq).

suppose that b(aq) is added to a solution of b at equilibrium.

a) will the equilibrium constant for the reaction increase, decrease, or stay the same? why?

b) will the concentration of hb+(aq) increase, decrease, or stay the same? why?

c) will the ph of the solution increase, decrease, or stay the same? why?

The answers are in the explanation

Explanation:

For the equilibrium:

B(aq) + H₂O(l) ⇌ HB⁺(aq) + OH⁻(aq).

By LeChatelier's principle, the increase in the concentration of a reactant (for example) at equilibrium will change the system counteracting the increasing producing more product.

Thus,

A) Will the equilibrium constant for the reaction increase, decrease, or stay the same? Why? .

The equilibrium constant is a thermodynamic constant that stay the same with the addition of a compound.

B) Will the concentration of HB⁺(aq) increase, decrease, or stay the same? Why?

By LeChatelier's principle, the addition of B will induce the formation of more HB⁺(aq) increasing the concentration.

C) Will the pH of the solution increase, decrease, or stay the same? Why?

As the addition of B induce the increasing of OH⁻, the pH of the solution will increase.

I hope it helps!

n+h→nh3

we must remember that nitrogen and hydrogen are both diatomic molecules in their standard gas form. this adjusts the equation to

n2+h2→nh3

now we need to adjust coefficients in order to balance the atoms on each side of the equation. currently we have 2 atoms of nitrogen and 2 atoms of hydrogen on the reactant side and 1 atom of nitrogen and 3 atoms of hydrogen on the product side.

we can balance the hydrogens by placing a coefficient of 2 in front of ammonia and a coefficient of 3 in front of the hydrogen.

n2+3h2→2nh3

this gives us 6 hydrogen on each side and coincidentally the nitrogens now equal 2 on each side.