Nickel nitrate and potassium carbonate react to form nickel carbonate and potassium nitrate. How many milliliters of 0.55M Ni(NO3)2 are needed to react with 85 mL of 0.25M K2CO3?
You should post it as an equation instead, so that it's easier to understand your question.
+2539 Solution (and precipitates):
\(\text {Solve and balance the equation to determine the reaction ratio. }\\ \text{ }\\ Ni(NO_3)_2 + K_2CO_3 \Rightarrow NiCO_3 + 2KNO_3 \small \text { Note that the ratio is 1:1}\\ \small \text {Determine the number of moles in the solution of 85ml with a 0.55 molar concentration of potassium carbonate. }\\ 0.25 * 85*10^{-3} L = \small \text{moles of potassium carbonate }\\ \small \text{Divide this by the 0.55 molar concentration of nickel (II) nitrate }\\ 0.02125/0.55 = 0.0386 L \\ 38.6 \text{ml} \small \text { of 0.55 molar nickel (II) nitrate } \)
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Easy as pealing a high potassium banana
GA
