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i upuriy Valdnice (atoms and charge). Make sus balanced cation and anion charge. Label the solids...
Please write the net ionic reaction only for every reaction and complete every box. If there is no reaction, please write NR. Thank you. 2) Rewrite the net ionic reaction on the page below. Example: Notebook Rxn: (AgNO, + NaCl): Total: Ag" (aq) + NO: (aq) + Na" (aq) + Cl(aq) → AgCl(s) + Na'(aq) + NO, (aq) Net: Ag" (aq) + Cl(aq) → AgCl(s) Page below Rxn: (AgNO, + NaCl): Ag*(aq) + Cl(aq) → AgCl(s) 3) If there is...
please help me find the cation and anion nominal concentrations for columns 4 and 5. the original solutions used as sources of ions are all 0.20 M. I'd appreciate if you showed the process as well as the answers. thank you! no equilibrium constant was given. It says the dilution equation must be used to determine the the nominal concentrations. Solutions Mixed Cation Anion Solution Solution Concentrations [Cation] [Anion] AgNO3 NaCI 0.10 0.10 AgNO3 KI AgNO3 Na2SO4 BaCl2 NaCl 0.10...
Name: 1.00g NaCl Volume: 100.34 mL Species (aq) a) The solution labeled 'Solution 1' contains 2.00 g NaCl. How many grams of AgNO3 must be added to the solution to the solution to completely react with NaCl according to the reaction in the background section? Molarity 1.00481e-7 1.00481e-7 0.170529 0.170529 OH Na CI Record the values for the concentration (molarity) for the Nat and Cl' species. 1. Calculate the number of grams of each species and please show work. Name:...
i need help on question 2a,b,c and 3a,b,c on the post lab. Experiment EQ-309 Post-Lab Questions Determination Of An Equilibrium Constant (To be answered in the "Analysis" section of your lab report) 1 a) Calculate the molarity of the silver nitrate solution provided. b) Calculate the molarity of the sodium chloride solution provided. 2 a) Use the data from each titration to calculate the value of K for the reaction, Ag(NH)2+ + Cl" - AgCl, + 2 NH, b) Calculate...
RODOX EXAMINATION An oxidation-reduction reaction involves the (1) sharing of electrons (3) transfer of electrons (2) sharing of protons (4) transfer of protons In this reaction, CO→ 2 CO + O2 the oxidation number of carbon changes from: (1) 0 to +4 (3) +3 to 0 (2) +2 to +4 (4) +4 to +2 Which balanced equation represents a redox reaction? AgNO3 (aq) +NaCl (aq) →AgCl (s) +NaNO3 (aq) H2CO3 (aq)...
When you write the answers, please write the page number for which the question is located. Thank you! Experiment 8 Name: Double Replacement Reactions Background: Some reactions have the net effect of causing the cation of cach reactant to trade places, forming a compound with the other anion. These reactions are known as double replacement reactions. In the example below (unbalanced equation), the barium and sodium cations switch places so that barium forms a product with sulfate while sodium forms...
Experiment 8 Double Replacement Reactions Background: Some reactions have the net effect of causing the cation of each reactant to trade places, forming a compound with the other anion. These reactions are known as double replacement reactions. In the example below (unbalanced equation), the barium and sodium cations switch places so that barium forms a product with sulfate while sodium forms a product with chloride. Note that the formula of each product is determined by the charges of the ions,...
What is the coefficient of H.So, when the following equation is properly balanced with the smallest set of whole numbers? __Cas(PO4h + H2SO4 - Caso + HPO. A) 3 B) 8 C) 10 D) 11 2) What is the coefficient of H20 when the following equation is properly balanced with smallest set of whole numbers? ALC + H2O - AM(OH), + CHE A) 3 B) 4 C) 6 D) 12 E) 24 3) of the reactions below, which one is...
I wasn't given the partial pressures so why do you need it? can the problem really not be solved without it? 1 bar for each 4. (11.11) The combustion of hydrogen is a reaction that is known to "go to completion." a. Use data in Appendix H to evaluate the thermodynamic equilibrium constant at 298.15 K for the reaction H2(g) + {O2(g) → H2O(1) b. Assume that the reaction is at equilibrium at 298.15 K in a system in which...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution of NaCl be used instead of NaNO3? 7. What was the purpose of FeSO4 solution in this experiment? 8. Could a solution of FeCl, be used instead of FeSO4? 9. Could a solution of NaSO4 be used instead of FeSO4? 10. Calculate the standard cell potential for the spontaneous redox reaction between a Pb(s)/Pb(NO3)2(aq) half-cell and a Ag(s)/AgNO3(aq) half-cell. Which metal would be oxidized?...