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A student needs to prepare 100. mL of 0.612 M Cu(NO3)2 solution. What mass, in grams, of copper(II) nitrate should the student use? Enter a numerical value with the correct number of significant figures in the answer box. Do not enter units, but know that the final units must be grams.

Respuesta :

Answer: 11.5 grams

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution

[tex]Molarity=\frac{n\times 1000}{V_s}[/tex]

where,

Morality = 0.612 M

n= moles of solute  

[tex]V_s[/tex] = volume of solution in ml = 100 ml

Now put all the given values in the formula of molarity, we get

[tex]0.612=\frac{n\times 1000}{100ml}[/tex]

[tex]n=0.0612moles[/tex]

[tex]Mass={\text {moles of solute }}{\times {\text {molar mass}}=0.0612moles\times 187.56g/mol=11.5g[/tex]

Therefore, the mass of copper (II)nitrate required is 11.5 grams

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The mass, in grams of copper(II) nitrate that the student should use to prepare 100. mL of 0.612 M Cu(NO3)2 solution is 11.48g.

HOW TO CALCULATE MASS:

  • The mass of a substance can be calculated by multiplying the number of moles of the substance by its molar mass.

  • According to this question, a student needs to prepare 100. mL of 0.612 M Cu(NO3)2 solution. The number of moles of copper II nitrate in the solution can be calculated as follows:

  • 100mL = 0.1L

  • no. of moles = volume × molarity

  • no. of moles = 0.1 × 0.612

  • no. of moles = 0.0612mol

  • Molar mass of Cu(NO3)2 = 187.56 g/mol

  • mass of Cu(NO3)2 = 0.0612 × 187.56

  • mass of Cu(NO3)2 = 11.48g

Therefore, the mass, in grams of copper(II) nitrate that the student should use to prepare 100. mL of 0.612 M Cu(NO3)2 solution is 11.48g.

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