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Yakvenalex [24]
3 years ago
13

Calculate pCl for the titration of 100.0mL of 0.1000 MCI with 0.1000 M

Chemistry
1 answer:
Anna71 [15]3 years ago
4 0

the titration is the most important part in determining whether

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Atoms of _______ gain electrons to fill their outer electron shells and become ________ ions.
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The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ________.
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Molecular equation:
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Complete ionic equation:

2H^{+}+SO_{4}^{2-} + 2Na^{+} +2OH^{-}--\ \textgreater \  2Na^{+}+SO_{4}^{2-} + 2H_{2}O(l)


Near 2H^{+},SO_{4}^{2-} ,  2Na^{+} , OH^{-} 

should be written (aq).

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8 0
3 years ago
If you need 0.0592 moles of nitrogen, how many grams of nitrogen do you need to mass(weigh) on the
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8 0
2 years ago
A container holds 6.4 moles of gas. Hydrogen gas makes up 25% of the total moles in the container. If the total pressure is 1.24
Degger [83]
  The   partial  pressure of hydrogen is 0.31  atm

calculation

find the number of  hydrogen   moles the container, that is

25/100  x 6.4  =1.6 moles of hydrogen

find the  partial pressure for hydrogen  in 1.6 moles

that is   6.4  moles=  1.24 atm
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by  cross  multiplication

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3 years ago
How many moles are found in a 100.0-g sample of CuF2?
ivolga24 [154]
To determine the amount of a substance in units of moles from units of grams, we need to determine the molar mass of the substance. <span>The </span>molar mass<span> is the </span>mass<span> of a given chemical element or chemical compound (g) divided by the amount of substance (mol). For CuF2, the molar mass </span><span>101.543 g/mol. We calculate as follows:

100.0 g CuF2 ( 1 mol / 101.543 g) = 0.98 mol CuF2</span>
6 0
3 years ago
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