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3 years ago

Suppose 1.87g of nickel(II) bromide is dissolved in 200.mL of a 52.0mM aqueous solution of potassium carbonate.

Chemistry

1 answer:

Reika [66]3 years ago

7 0

Answer:

0.0428 M

Explanation:

Because we're asked to calculate the molarity of nickel(II) cation, we need to <u>determine all sources for that species</u>, in this case, all Ni⁺² comes from the nickel(II) bromide solid (NiBr₂).

We use the molecular weight of NiBr₂ to calculate the moles of Ni:

1.87 g NiBr₂ ÷ 218.49g/mol * (1molNi⁺²/1molNiBr₂) = 8.55x10⁻³ mol Ni⁺²

Then we <u>divide the moles by the volume in order to calculate the concentration</u>:

8.55x10⁻³ mol Ni⁺² / 0.200 L = 0.0428 M

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Answer:

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Explanation:

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IrinaK [193]

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Explanation:

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