To completely react 17g of barium hydroxide, how many grams of hydrochloric acid is needed?
Ba(OH)2 + 2HCl ==> BaCl2 _ 2H2O
mols Ba(OH)2 = grams/molar mass = ?
Using the coefficient sin the balanced equation, convert mols Ba(OH)2 to mols HCl.
Now convert mols HCl to grams. grams = mols HCl x molar mass HCl.
To determine the amount of hydrochloric acid needed to completely react with 17g of barium hydroxide, we need to use the balanced chemical equation for the reaction between barium hydroxide (Ba(OH)2) and hydrochloric acid (HCl).
The balanced equation is:
Ba(OH)2 + 2HCl -> BaCl2 + 2H2O
From the equation, we can see that one mole of barium hydroxide reacts with two moles of hydrochloric acid to produce one mole of barium chloride and two moles of water.
1 mole Ba(OH)2 = 171.34g
2 moles HCl = 2 * 36.46g = 72.92g
Now, we can set up a proportion to calculate the mass of hydrochloric acid needed:
(17g Ba(OH)2) / (1 * 171.34g Ba(OH)2) = (xg HCl) / (72.92g HCl)
By cross-multiplying, we get:
17g Ba(OH)2 * 72.92g HCl = 1 * 171.34g Ba(OH)2 * xg HCl
x = (17g * 72.92g HCl) / (1 * 171.34g) ≈ 7.21g
Therefore, approximately 7.21 grams of hydrochloric acid is needed to completely react with 17 grams of barium hydroxide.