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if you had 100 mL of 0.1 M Na2CO3, how many mL of 1 M MgSO4 would you need to add in order to use up hoth reactants, without either being leftover?

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With 100 mL, 0.1M [tex]Na_2CO_3[/tex], the volume of 1M [tex]MgSO_4[/tex] that would be needed for complete reaction will be 0.01 L or 10 mL

Stoichiometric calculations

The equation of the reaction is as follows:

[tex]Na_2CO_3 + MgSO_4 ---- > Na_2SO_4 + MgCO_3[/tex]

Both reactants are in the ratio 1:1.

Mole = molarity x volume

Mole of 100mL, 0.1M  [tex]Na_2CO_3[/tex] = 0.1 x 0.1 = 0.01 moles

Equivalent mole of  [tex]MgSO_4[/tex] will also be 0.01  moles.

Volume of 0.01 moles, 1M [tex]MgSO_4[/tex] = 0.01/1 = 0.01 L or 10 mL

More stoichiometric calculations can be found here: https://brainly.com/question/27287858

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