When 5.88 g of CaO(s) is completely dissolved by HBr(aq), how many grams of CaBr2(aq) form in solution?
Step 1 of 3
Here we have to calculate the mass of CaBr2(aq) form in solution.
Mass of CaO = 5.88 g
CaO + 2HBr CaBr2 + H2O
Moles = mass solute/ molecular mass = 5.88/ 56.0774 = 0.104 moles
1 mole of CaO has formed 1 mole of CaBr2(aq)
Thus the ratio is 1:1 of CaO:CaBr2
Hence 0.104 moles of CaBr2 produced 200g/mole = 20.8g CaBr2 produced
Thus 20.8 g of CaBr2 has produced
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
Since the solution to 94P from 14 chapter was answered, more than 860 students have viewed the full step-by-step answer. This full solution covers the following key subjects: cabr, Cao, completely, Dissolved, form. This expansive textbook survival guide covers 19 chapters, and 2046 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 94P from chapter: 14 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. The answer to “When 5.88 g of CaO(s) is completely dissolved by HBr(aq), how many grams of CaBr2(aq) form in solution?” is broken down into a number of easy to follow steps, and 18 words. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5.