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Monica [59]
3 years ago
8

According to the label on a bottle of concentrated hydrochloric acid, the contents are 36% by mass and have a density of 1.138g/

mL. What mass (in Kg) of sodium hydrogen carbonate would be needed to neutralize the spill if a bottle containing 1.508L of concentrated HCl dropped on the lab floor and broke open?
Chemistry
1 answer:
elixir [45]3 years ago
7 0

Answer:

1.42 Kg of NaHCO3

Explanation:

From

Co= 10 pd/M

Where;

Co= concentration of the stock solution of acid

p= percentage of raw acid = 36%

d= density of the acid= 1.138g/mL

M= molar mass of the acid= 36.5 g/mol

Co= 10 × 36 × 1.138/36.5

Co= 11.22 M

Number of moles of acid= CV = 11.22 M × 1.508 L= 16.9 moles

The reaction equation is;

NaHCO3(aq)+HCl(aq)→NaCl(aq)+H2O(l)+CO2(g)

If 1 mole of NaHCO3 reacts with 1 mole of HCl

Then 16.9 moles of HCl reacts with 16.9 moles of NaHCO3

Hence 16.9 moles of NaHCO3 is required to neutralize the HCl.

From

n= m/ M

Where;

n= number of moles = 16.9

m= mass of NaHCO3= ??

M= molar mass of NaHCO3= 84.007 g/mol

m= n× M/1000

m= 16.9 × 84.007 /1000

m= 1.42 Kg

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The specific heat of the unknown metal is 0.859 J/g⁰C.

<h3>Specific heat of the unknown metal</h3>

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Answer:

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Explanation:

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In this case, since the molarity of a solution is computed by dividing the moles of solute by the volume of solution in liters, we first need to compute the moles of solute knowing that the molar mass of calcium hydroxide is 74.1 g/mol as follows:

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Next, since the 100-mL solution is also expressed in liters by 0.100 L, we directly compute the molarity as shown below:

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