Chemistry, 29.07.2019 12:50 robert7248

Why is insoluble salt washed with distilled water

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Answer from: mia1518

For illustration, you want to prepare a pure sample of CaCO3. This is often done in the pharmaceutical industry for the production of CaCO3 filler used in tablets and antacids.
You can do this by mixing solutions of CaCl2 and Na2CO3
CaCl2(aq) + Na2CO3(aq) →CaCO3(s) + 2NaCl(aq)
The CaCO3 preciitates as a very fine precipitate. The NaCl solution is drained away. Any NaCl adhering to the CaCO3 is removed by further washing of the precipitate and recovering the CaCO3 by filtration. For this to be effective, the NaCl has to be readily soluble in water, which it is.
You cannot have reactions occuring where the two reactants are insoluble in the water, and it is unusual, but not unknown, to produce two precipitates from the single reaction.

Hope this helps!

Answer from: Quest

1.consider the following balanced equation and answer parts a through. show calculations for each part.

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.

explanation:

Answer from: Quest

i don,t know so just answer mine

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