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Inga [223]
3 years ago
5

The molar mass of Ba(OH)2 is (1) 154.3 g (3) 171.3 g (2) 155.3 g (4) 308.6 g

Chemistry
1 answer:
Archy [21]3 years ago
8 0
Ba(OH)₂ = 137.3 + 16 x 2 + 1 x 2 = 171.3 g

Answer (3)

hope this helps!

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20 mL of Ba(OH)2 solution with unknown concentration was neutralized by the addition of 43.89 mL of a .1355 M HCl solution. Calc
bezimeni [28]

Answer:

Concentration of the barium ions  = [Ba^{2+}] = 0.4654 M

Concentration of the chloride ions  = [Cl^{-}]=0.9308 M

Explanation:

Moles (n)=Molarity(M)\times Volume (L)

Moles of hydrogen chloride = n

Volume of hydrogen chloride solution = 43.89 mL = 0.04389 L

Molarity of the hydrogen chloride  = 0.1355 M

n=0.1355 M\times  0.04389 L=0.005947 mol

Ba(OH)_2+2HCl\rightarrow BaCl_2+2H_2O

According to reaction, 2 moles of HCl reacts with 1 mole of barium hydroxide.

Then 0.05947 moles of HCl will react with:

\frac{1}{2}\times 0.05947 mol=0.029735 mol barium hydroxide

Moles of barium hydroxide = 0.029735 mol

Ba(OH)_2(aq)\rightarrow Ba^{2+}(aq)+2OH^-(aq)

1 mole of barium hydroxide gives 1 mole of barium ion in an aqueous solution. Then 0.029735 moles of barium hydroxide will give:

=1\times 0.029735 mol= 0.029735 mol

Volume of solution after neutralization reaction :

= 20.0 mL + 43.89 mL  = 63.89 mL = 0.06389 L

Concentration of the barium ions =[Ba^{2+}]

[Ba^{2+}]=\frac{0.029735 mol}{0.06389 L}=0.4654 M

Ba(Cl)_2(aq)\rightarrow Ba^{2+}(aq)+2Cl^-(aq)

1 mole of barium chloride gives 1 mole of barium ions and 2 moles of chloride ions in an aqueous solution.

Then concentration of chloride ions will be:

[Cl^-]=2\times [Ba^{2+}]=2\times 0.4654 M=0.9308 M

8 0
3 years ago
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