Which gas law would you use for the following problem: What pressure is required to hold 8.0 moles of oxygen gas in an 8.0 L con
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Answer:
7.32g of HNO3 are required.
Explanation:
1st) From the balanced reaction we know that 2 moles of HNO3 react with 1 mole of Ca(OH)2 to produce 2 moles of H2O and 1 mole of Ca(NO3)2.
From this, we find that the relation between HNO3 and Ca(OH)2 is that 2 moles of HNO3 react with 1 mole of Ca(OH)2.
2nd) This is the order of the relations that we have to use in the equation to calculate the grams of nitric acid:
• starting with the 4.30 grams of Ca(OH)2.
,• using the molar mass of Ca(OH)2 (74g/mol).
,• relation of the 2 moles of HNO3 that react with 1 mole of Ca(OH)2 .
,• using the molar mass of HNO3 (63.02g/mol).
So, 7.32g of HNO3 are required.
Answer : The mass of sulfuric acid needed is .
Solution : Given,
pH = 8.94
Volume of solution = 380 ml =
Molar mass of sulfuric acid = 98.079 g/mole
As we know,
Now we have to calculate the moles of .
Formula used :
For neutralization, equal number of moles of ions will neutralize same number of
ions.
As,
From this reaction, we conclude that
2 moles of ion is given by the 1 mole of
moles of
ion is given by
moles of
Now we have to calculate the mass of sulfuric acid.
Mass of sulfuric acid = Moles of × Molar mass of sulfuric acid
Mass of sulfuric acid =
Therefore, the mass of sulfuric acid needed is .