Suppose of nickel (II) bromide is dissolved in of a aqueous solution of potassiu

Question

Suppose of nickel (II) bromide is dissolved in of a aqueous solution of potassium carbonate. Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the nickel (II) bromide is dissolved in it. Round your answer to significant digits.

Explanation / Answer

find moles, using molar mass: 2.71 g ZnCl2 @ 136.32 g ZnCl2 / mole = 0.01988 moles Zn+2 find moles 0.350.L @ 0.0560 moles / Litre = 0.0196 moles (CO3)-2 by the equation Zn+2 & CO3)-2 --> ZnCO3 (s) 0.0196 moles (CO3)-2 reacts with an equal 0.0196 moles Zn+2 , 0.01988 moles Zn+2 - 0.0196 moles Zn+2 reacted = 0.00028 moles Zn+2 remain find molarity remaining 0.00028 moles Zn+2 / 0.350 litres = 0.000799 Molar your answer, to 1 sig fig is 0.0008 Molar Zn+2 aka 0.8 milliMolar Zn+2

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