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Alex17521 [72]
3 years ago
12

46.0 g of barium nitrate is dissolved in 360 g of water. What is the percent concentration of the barium nitrate solute in the s

olution?
Pls help with answer I don’t get it
Chemistry
1 answer:
avanturin [10]3 years ago
8 0

The percent concentration of the Barium nitrate : 11.33%

<h3>Further explanation</h3>

The concentration of a substance can be expressed in several quantities such as moles, percent (%) weight/volume,), molarity, molality, parts per million (ppm) or mole fraction. The concentration shows the amount of solute in a unit of the amount of solvent.

\tt \%mass=\dfrac{mass~solute}{mass~solution}\times 100\%

mass solute=mass Barium nitrate(Ba(NO₃)₂)=46 g

mass solvent=mass water=360 g

mass solution=mass solute+mass solvent=46+360=406 g

\tt \%mass=\dfrac{46}{406}\times 100\%\\\\\%mass=\boxed{\bold{11.33\%}}

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Conditioning two or three times will insure that the concentration of titrant is not changed by a stray drop of water.

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A solution is prepared by dissolving 0.23 mol of lactic acid and 0.27 mol of sodium lactate in water sufficient to yield 1.00 L
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Explanation:

The solution of the lactic acd and sodium lactate is referred to as a buffer solution.

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Buffer solutions are generally known to resist change in pH values.

When a strong base (in this case, NaOH) is added to the buffer, the lactic acid will give up its H+ in order to transform the base (OH-) into water (H2O) and the conjugate base, so we have:

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3 years ago
A chemist dissolves 797. mg of pure barium hydroxide in enough water to make up 60. mL of solution. Calculate the pH of the solu
topjm [15]

Answer:

13.20

Explanation:

Step 1: Calculate the moles of Ba(OH)₂

The molar mass of Ba(OH)₂ is 171.34 g/mol.

0.797 g × 1 mol/171.34 g = 4.65 × 10⁻³ mol

Step 2: Calculate the molar concentration of Ba(OH)₂

Molarity is equal to the moles of solute divided by the liters of solution.

[Ba(OH)₂] = 4.65 × 10⁻³ mol/60 × 10⁻³ L = 0.078 M

Step 3: Calculate [OH⁻]

Ba(OH)₂ is a strong base according to the following equation.

Ba(OH)₂ ⇒ Ba²⁺ + 2 OH⁻

The concentration of OH⁻ is 2/1 × 0.078 M = 0.16 M

Step 4: Calculate the pOH

pOH = -log OH⁻ = -log 0.16 = 0.80

Step 5: Calculate the pH

We will use the following expression.

pH + pOH = 14

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