4. What is the net ionic equation for the following reaction? (2 Pts.) K2CO3 (aq) +...
5. An unknown gas has a density of 0.355 g/L at 17 °C and 189 mm Hg. (i) Calculate the molar mass of the gas? (ii) What is the identity of the gas? (2 pts.)
23. Write a complete ionic and net-ionic equation for the following reaction. K2CO3(aq) + H2SO4 (aq) → 24. a) What volume(ml) of 0.115 M HCIO4 solution is required to neutralize 50.00 ml of 0.0875 M Ca(OH)2 ? b) A solution contains 3.2 g NaOH (MW = 40) in 20.0 ml of solution. What is the molarity of the solution? 25. A 44.0 g sample of an unknown metal at 99.0 °C was placed in a constant pressure calorimeter of negligible...
What are the product of the following reaction? H2SO4(aq) + K2CO3(aq) O H2CO2(aq) + KSO4(aq) O H2CO3(aq) + KSO4(aq) H20(1) + K2SO4(aq) + CO2(g) O H2(g) + CO2(g) + K2SO4(aq)
Write the complete ionic equation and the net ionic equation for each of the reactions: Co(NO3)2(aq) + K2CO3(aq) --> CoCO3(s) + 2KNO3(aq) AgNO3(aq) + CsI(aq) ---> AgI(s) + CsNO3(aq) KHCO3(aq) + KOH(aq) --> K2CO3(aq) + H2O(l) H2SO4(aq) + 2NH3(aq) --> (NH4)2SO4(aq) 3Mg(s) + 2FeCl3(aq) --> 3MgCl2(aq) + 2Fe(s)
Enter the balanced complete ionic equation for HCl(aq)+K2CO3(aq)→H2O(l)+CO2(g)+KCl(aq). Express your answer as a chemical equation. Identify all of the phases in your answer.
Reaction in Aquesous 1. Write the balanced molecular equation, complete ionic equation, and net ionic equation for the following: (5 pts) HI + K2CO3 → Complete ionic equation: Net ionic equation: TURN OVER → 2. A 31.5mL aliquot of H2SO4 of unknown concentration was titrated with 0.0134M NaOH. It took 23.9mL of NaOH to reach the endpoint of the titration. What is the concentration of the H2SO4? (5 pts) 3. In the following reaction, indicate the substance being oxidized, reduced,...
what is the total ionic (not net) equation of 2KAl(OH)4(aq)+H2SO4(aq)=2Al(OH)3(s)+K2SO4(aq)+2H2O(l)
1(i). Balance the following equations, and then write the net ionic equation (a) (NH4)2CO3(aq) + Cu(NO3)2(aq) → CuCO3(s) + NH4NO3(aq) (b) Mg(OH)2(s) + HCl(aq) → MgCl2(aq) + H2O(l) (c) BaCO3(s) + HBr(aq) → BaBr2(aq) + H2O(l) + CO2(g) (ii). For each reaction equation, identify the driving force of the reaction 2. What is an electrolyte? How can you experimentally differentiate between a weak electrolyte and a strong electrolyte? Name and give the formulas of a strong electrolyte and a weak...
Write the net ionic equation and describe the reactions occurring. 1) 2 KAl(OH)4(aq) + H2SO4(aq) ----> 2 Al(OH)3(s) + K2SO4(aq) + 2 H2O(l) 2) 2 Al(OH)3(s) + [6 H+ + 3 SO2-4(aq) ----> [2 Al3+ + 3SO2-4](aq) + 6H2O(l) The following is a bank for the types of reactions that can be occurring. Two or more can be present in one equation. Metathesis Reactions Redox Reactions Single Displacement Reactions Double Displacement Reactions Combination Reactions Decomposition Reactions
Write the complete ionic and net ionic equations for each of the following reactions: To write complete ionic equations and net ionic equations follow the steps below: (I) Write the molecular equation and balance it. (II) Determine the state of each substance(gas, liquid, solid, aqueous). Use the solubility rules! (III) Write the ionic equation by breaking all the soluble ionic compounds (those marked with an (aq) into their respective ions. (IV) Write the net ionic equation by removing the spectator...