Open Question
Complete and balance each gas-evolution equation. b. HCl(aq) + KHCO3(aq) → c. HC2H3O2(aq) + NaHSO3(aq) → d. (NH4)2SO4(aq) + Ca(OH)2(aq) →
Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 12
We prepare a solution by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L of a 0.18 M MgCl2 solution. What volume of a 0.20 M silver nitrate solution is needed to precipitate all the Cl- ions in the solution as AgCl?
Verified step by step guidance1
Calculate the moles of Cl- ions from the NaCl solution using the formula: \( \text{moles} = \text{volume} \times \text{molarity} \).
Calculate the moles of Cl- ions from the MgCl2 solution. Remember that each mole of MgCl2 provides 2 moles of Cl- ions.
Add the moles of Cl- ions from both solutions to find the total moles of Cl- ions present.
Use the stoichiometry of the reaction between Cl- ions and Ag+ ions to determine the moles of Ag+ needed. The reaction is: \( \text{Ag}^+ + \text{Cl}^- \rightarrow \text{AgCl} \).
Calculate the volume of 0.20 M AgNO3 solution required to provide the necessary moles of Ag+ ions using the formula: \( \text{volume} = \frac{\text{moles}}{\text{molarity}} \).
Related Practice
Open Question
Complete and balance each combustion reaction equation: a. C(s) + O2(g) → b. C3H8O(l) + O2(g) → c. CS2(s) + O2(g) → d. C4H6(g) + O2(g) →
Open Question
Consider the balanced equation: 2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g). Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms. Mol N2H4 Mol N2O4 Mol N2 Mol H2O 2 _____ _____ _____ _____ 5 _____ _____ _____ _____ _____ 10 _____ _____ 11.8 _____ 2.5 _____ _____ _____ _____ 4.2 _____ _____
Open Question
Consider the unbalanced equation for the combustion of hexane: C6H14(g) + O2(g) → CO2(g) + H2O(g). Balance the equation and determine how many moles of O2 are required to react completely with 7.2 moles of C6H14.
Textbook Question
Consider the unbalanced equation for the neutralization of acetic acid: HC2H3O2(aq) + Ba(OH)2(aq) → H2O(l) + Ba(C2H3O2)2(aq) Balance the equation and determine how many moles of Ba(OH)2 are required to completely neutralize 0.461 mole of HC2H3O2.
1998
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Open Question
Calculate how many moles of NO2 form when each quantity of reactant completely reacts.
Reaction: 2 N2O5(g) → 4 NO2(g) + O2(g)
a. 15.2 g N2O5
b. 6.8 mol N2O5
c. 2.87 kg N2O5