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Dimas [21]
4 years ago
8

If it requires 18.2 milliliters of 0.45 molar barium hydroxide to neutralize 38.5 milliliters of nitric acid, solve for the mola

rity of the nitric acid solution. Show all of the work used to solve this problem. Unbalanced equation: Ba(OH)2 + HNO3 yields Ba(NO3)2 + H2O
Chemistry
2 answers:
Elina [12.6K]4 years ago
7 0

Answer: 0.42 M

Explanation:

Ba(OH)_2+2HNO_3\rightarrow Ba(NO_3)_2+2H_2O

The expression used will be :

n_1M_1V_1=n_2M_2V_2

where,

n_1 = basicity of HNO_3 = 1

n_2 = acidity of Ba(OH)_2 = 2

M_1 = concentration of HNO_3 = ?

M_2 = concentration of Ba(OH)_2 = 0.45 M

V_1 = volume of HNO_3 = 38.5 ml

V_2 = volume of Ba(OH)_2 = 18.2 ml

Now put all the given values in the above law, we get the concentration:

(1\times M_1\times 38.5)=(2\times 0.45M\times 18.2ml)

By solving the terms, we get :

M_1=0.42M

Therefore, the concentration of HNO_3 is 0.42M

Ghella [55]4 years ago
5 0
Hi! :)

Ba(OH)2 + 2 HNO3 → Ba(NO3)2 + 2 H2O

(18.2 mL) x (0.45 M Ba(OH)2) x (2 mol HNO3 / 1 mol Ba(OH)2) / (38.5 mL HNO3) = 0.43 M HNO3
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Answer:

\large \boxed{\text{21.6 L}}

Explanation:

We must do the conversions

mass of C₆H₁₂O₆ ⟶ moles of C₆H₁₂O₆ ⟶ moles of CO₂ ⟶ volume of CO₂

We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ:        180.16

         C₆H₁₂O₆ + 6O₂ ⟶ 6CO₂ + 6H₂O

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\text{Moles of CO}_{2} =\text{0.1360 mol C$_{6}$H$_{12}$O}_{6} \times \dfrac{\text{6 mol CO}_{2}}{\text{1 mol C$_{6}$H$_{12}$O}_{6}} = \text{0.8159 mol CO}_{2}

(c) Volume of CO₂

We can use the Ideal Gas Law.

pV = nRT

Data:

p = 0.960 atm

n = 0.8159 mol

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(i) Convert the temperature to kelvins

T = (37 + 273.15) K= 310.15 K

(ii) Calculate the volume

\begin{array}{rcl}pV &=& nRT\\\text{0.960 atm} \times V & = & \text{0.8159 mol} \times \text{0.082 06 L}\cdot\text{atm}\cdot\text{K}^{-1}\text{mol}^{-1} \times \text{310.15 K}\\0.960V & = & \text{20.77 L}\\V & = & \textbf{21.6 L} \\\end{array}\\\text{The volume of carbon dioxide is $\large \boxed{\textbf{21.6 L}}$}

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