Question

Explain how to make at least one liter of a 1.25 molar ammonium hydroxide solution?

Answer 1

Answer:

M=1.25mol/L

M.M. of NH₄OH=14+5+16=35g

Volume=1L

As, M=m÷[M.M.×V(L)]

⇒m=M×M.M.×V

=1.25×35×1

∴ m=43.75g

Therefore, for making a solution of Ammonium hydroxide, with molarity of 1.25M in 1L of solution, you mist dissolve 43.75g of NH₄OH

Answer 2

Given: Volume - V = 1L

            Molarity - M = 1.25M ( ammonium hydroxide- NH₄OH)

To Find:

mass -m of NH₄OH to mix with 1L water to form the solution.

Solution:

Formula used: Molarity = moles of solute(n)/V (in L)

n = m/molecular mass of solute(NH₄OH) - M

Molecular mass of NH₄OH = 14 + 4 + 16 +1 = 35g

Applying the above formulas:

M = m/MₓV

m = M ₓ V ₓ M

m = 1.25 ₓ 1 ₓ 35

m = 43.75g

∴ 1 L of water added to 43.75g of NH₄OH