Based on your observation, how would you precipitate BaCrO4 (s) from a solution of Ba(NO3)2 and K2Cr2O7 2-? Need to show chemical equation and explain.
From the question I assume you did an experiment of some kind and made some observations. What were those observations?
I saw yellow thick cloudy liquid but no precipitate
To precipitate BaCrO4 (s) from a solution of Ba(NO3)2 and K2Cr2O7, you can use a double displacement reaction where barium ions and chromate ions combine to form a precipitate. Here are the steps:
Step 1: Write the balanced chemical equation for the reaction.
Ba(NO3)2 (aq) + K2Cr2O7 (aq) → BaCrO4 (s) + KNO3 (aq)
Step 2: Identify the ions present in the reactants and products.
- Ba(NO3)2 dissociates into Ba2+ and 2(NO3-) ions.
- K2Cr2O7 dissociates into 2K+ and Cr2O7^2- ions.
- The product BaCrO4 is a precipitate (insoluble in water), so it becomes a solid in the equation.
- KNO3 dissociates into K+ and NO3- ions.
Step 3: Determine the driving force for the precipitation reaction.
The driving force for the precipitation reaction is the formation of an insoluble compound, BaCrO4. When the chromate ions (Cr2O7^2-) react with barium ions (Ba2+), they form BaCrO4 as a solid, which is less soluble and precipitates out of the solution.
Step 4: Balance the equation.
2Ba(NO3)2 (aq) + K2Cr2O7 (aq) → BaCrO4 (s) + 2KNO3 (aq)
Step 5: Verify the equation's balance and net ionic equation.
In the equation above, we have balanced both the ions and atoms on both sides. The net ionic equation is obtained by removing the spectator ions (ions that do not participate in the reaction) from the complete ionic equation. In this case, the spectator ions are NO3- and K+.
Net ionic equation:
Ba2+ (aq) + Cr2O7^2- (aq) → BaCrO4 (s)
So, by mixing solutions of Ba(NO3)2 and K2Cr2O7, you can precipitate BaCrO4 (s) by forming an insoluble compound, BaCrO4, through a double displacement reaction.
To precipitate BaCrO4 (barium chromate) from a solution of Ba(NO3)2 (barium nitrate) and K2Cr2O7 (potassium dichromate), you will need to perform a double displacement reaction. Here is the step-by-step explanation:
1. Write out the balanced chemical equation for the reaction between Ba(NO3)2 and K2Cr2O7:
Ba(NO3)2(aq) + K2Cr2O7(aq) → BaCrO4(s) + 2KNO3(aq)
2. In this reaction, the cations Ba2+ from Ba(NO3)2 and the anions CrO42- from K2Cr2O7 will combine to form the insoluble BaCrO4 precipitate.
3. The balanced equation indicates that for each molecule of Ba(NO3)2 and K2Cr2O7, one molecule of BaCrO4 will be formed.
4. In practice, to precipitate BaCrO4:
a. Combine the Ba(NO3)2 solution with the K2Cr2O7 solution in a reaction vessel.
b. Stir the mixture to ensure complete mixing.
c. Observe the yellow precipitate of BaCrO4 forming.
5. Once the precipitate has formed, it can be collected by filtration, washed with deionized water to remove any impurities, and then dried for further use or analysis.
Remember, it is important to follow proper lab safety protocols and consult relevant literature or your instructor for specific instructions and precautions for this experiment.