Write the balanced molecular equation for the neutralization reaction between HI and Ba(OH), in aqueous solution. Include physical states. molecular equation:2HI(aq)+Ba(OH), (aq) → Bal, (aq) + 2H,O Incorrect
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- What is the product of the following reaction equation after balancing? If no reaction state that " Mg(s)+HCI(aq) ---->Balance the following in acidic medium: MnO4- + Fe2+ ---> Mn2+ + Fe3+ How many Fe2+ are there in the balanced equation?What is the % purity of a sample of oxalic acid if a 0.4006g sample requires 28.62mL of potassium permanganate solution, of which 1mL contains 5.98mg potassium permanganate? A. Write the chemical reaction showing the OS of each elementB. Show the half-reactions and balance the number of electrons lost and gainedC. Identify the reducing agent and the oxidizing agent and solve for their milliequivalent weightsD. Write the balanced equilibrium reactionE. Show your solution for % purity; the answer is 85.2%
- A precipitate of AgCl + AgBr weighs 0.8132 g. On heating on a current of Cl2, the AgBr is converted to AgCl, the mixture loses 0.1450 g in wt. Find the percentage Cl in the original sample.Answer d to i:The purity of the salt Sn3(PO4)2 (546.0727), was determined by the redox titration with KMnO4. Half reactions involved:Unbalanced half reactions: MnO4- ↔ Mn2+Sn2+ ↔ Sn4+ a) Balance the redox reaction given above. b) Write the fundamental equation for the redox stoichiometry between Sn2+ and MnO4- Before analysis, KMnO4 solution was standardized according to the following procedure: 1.000 g of 100% pure tin, Sn (118.71) wire was used. After proper chemical treatment, a volume of 29.75 mL of the permanganate solution was used in the titration of the reduced tin. c) Calculate the concentration of the KMnO4 solution. An as received sample of the salt Sn3(PO4)2 (546.0727) weighing 5.0550 g was dissolved in water. The sample was treated to completely reduce all the tin to Sn2+. This solution was then titrated with standard KMnO4 (158.03) (calculated in (c)). 40.00 mL of the standard KMnO4 solution was used in the titration to reach the equivalence point. d) What is the purity…A precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is converted into AgCl, the mixture losing 0.1450 gram in weight. What was the percentage of chlorine in the original precipitate?
- a. Balance the following redox in acidic media C2O42- (aq) + MnO4- (aq) → CO2(aq) + Mn2+ (aq) b. If you titrated this reaction to determine the moles of C2O42-, the colormetric endpoint is pink due to the Mn2+. How many moles of the oxalate (C2O42-) existed in solution if 12 mL of 0.791M permanganate was needed to hit the endpoint?Which substance functions as a reducing agent in the following reaction CH4+ 2O2-->CO2+ 2H2OWhat is the Molarity of a NaOH solution of 25.0 ml of this NaOH solution is required to neutralize 20.0 ml of 0.30 M H2SO4 Write Balance equation to acertaron the stoichiometry of this reaction? explain me balance equation please!
- If you complete and balance the following equation in acidicsolutionMn2+(aq) + NaBiO3(s)---->Bi3+(aq)+ MnO4-(aq) + Na+(aq)how many water molecules are there in the balanced equation(for the reaction balanced with the smallest whole-numbercoefficients)? (a) Four on the reactant side (b) Three on the product side (c) One on the reactant side (d) Seven on theproduct side (e) Two on the product sidebalanced molecular equation (ME) write the balanced complete ionic equation (CIE) and write the balanced net ionic equation (NIE) Tin(II) chloride + potassium nitrate SnCl2(aq) KNO3(aq) Observations: No observable change; solution mixture is clear and colorless ME: CIE: NIE:A solution of hydrobromic acid is added to a solution of sodium hydroxide. Which of the following is true about the reaction between HBr and NaOH? SELECT ALL THAT APPLY! A. NaBr(aq) is formed as a product. B. The net ionic equation is: H+(aq) + OH-(aq) --> H2O(l) C. NaBr is a solid precipitate that forms. D. H2O (l) is formed as a product.