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Len [333]
3 years ago
14

Brass is an alloy of copper and zinc. varying the mass per- centages of the two metals produces brasses with different proper- t

ies. a brass called yellow zinc has high ductility and strength and is 34–37% zinc by mass. (a) find the mass range (in g) of copper in 185 g of yellow zinc. (b) what is the mass range (in g) of zinc in a sample of yellow zinc that contains 46.5 g of copper?
Chemistry
1 answer:
EastWind [94]3 years ago
7 0

First step: The mass of zinc in the yellow zinc sample can be calculated with the help of percentage (given) in the sample. After that, mass of copper is determine by the subtracting the mass of zinc from the total mass of zinc in the given sample.

Thus,

Mass of zinc in 34% zinc sample = 185 g yellow zinc \times \frac{34 zinc}{100 yellow zinc}

= 62.9 g zinc

Mass of zinc in 37% zinc sample = 185 g yellow zinc \times \frac{37 zinc}{100 yellow zinc}

= 68.45 g zinc

Now,

mass of copper in 34% zinc sample =185 g -62.9 g

= 122.1 g \simeq 122 g

mass of copper in 37% zinc sample = 185 g -68.45 g

=116.55 g \simeq 117 g

Thus, the range of mass of copper is 117 g to  122 g

Second step:

34% zinc sample consist of 66% copper (100-34= 66%)

37% zinc sample consist of 63% copper (100-37=63%)

Mass of zinc = (46.5 g copper) \times \frac{34 percent zinc}{66 percent copper}

= 23.95 g\simeq 24 g

Mass of zinc  =46.5 g copper \times \frac{37 percent zinc}{63 percent copper}

= 27.30 g\simeq 27g

Thus, the range of mass of zinc is 24 g to  27 g





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A sample of solid sodium hydroxide, weighing 13.20 grams is dissolved in deionized water to make a solution. What volume in mL o
Andreas93 [3]
<h3>Answer:</h3>

2.809 L of H₂SO₄

<h3>Explanation:</h3>

Concept tested: Moles and Molarity

In this case we are give;

Mass of solid sodium hydroxide as 13.20 g

Molarity of H₂SO₄ as 0.235 M

We are required to determine the volume of H₂SO₄ required

<h3>First: We need to write the balanced equation for the reaction.</h3>
  • The reaction between NaOH and H₂SO₄ is a neutralization reaction.
  • The balanced equation for the reaction is;

2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O

<h3>Second: We calculate the umber of moles of NaOH used </h3>
  • Number of moles = Mass ÷ Molar mass
  • Molar mass of NaOH is 40.0 g/mol
  • Therefore;

Moles of NaOH = 13.20 g ÷ 40.0 g/mol

                          = 0.33 moles

<h3>Third: Determine the number of moles of the acid, H₂SO₄</h3>
  • From the equation, 2 moles of NaOH reacts with 1 mole of H₂SO₄
  • Therefore, the mole ratio of NaOH: H₂SO₄ is 2 : 1.
  • Thus, Moles of H₂SO₄ = moles of NaOH × 2

                                    = 0.33 moles × 2

                                   = 0.66 moles of H₂SO₄

<h3>Fourth: Determine the Volume of the acid, H₂SO₄ used</h3>
  • When given the molarity of an acid and the number of moles we can calculate the volume of the acid.
  • That is; Volume = Number of moles ÷ Molarity

In this case;

Volume of the acid = 0.66 moles ÷ 0.235 M

                                = 2.809 L

Therefore, the volume of the acid required to neutralize the base,NaOH is 2.809 L.

7 0
3 years ago
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