Write the balanced NET ionic equation for the reaction when HCIO3 and Ba(OH)2 are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
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- Write a net ionic equation for the reaction between aqueous solutions of (a) ammonia and hydrofluoric acid. (b) perchloric acid and rubidium hydroxide. (c) sodium aulfite and hydriodic acid. (d) nitric acid and calcium hydroxide.What mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?(a) Write the net ionic equation for the reaction that occurswhen a solution of hydrochloric acid (HCl) is mixed with asolution of sodium formate (NaCHO2). (b) Calculate theequilibrium constant for this reaction. (c) Calculate theequilibrium concentrations of Na+, Cl-, H+, CHO2-, andHCHO2 when 50.0 mL of 0.15 M HCl is mixed with 50.0 mLof 0.15 M NaCHO2.
- (a) True or false: “solubility” and “solubility-product constant”are the same number for a given compound. (b) Writethe expression for the solubility-product constant for eachof the following ionic compounds: MnCO3, Hg(OH)2, andCu3(PO4)2.Question 22 of 30 Submit A 185.0 mL sample of 1.200 M Pb(NO3)2 is mixed with 123.50 mL of 1.500 M NaCI, and the PbCl, precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr, precipitate is also collected and dried. What is the mass (in grams) of the PbBr, precipitate, assuming the yield in each precipitation step is 100%? 1 4 6. C 7 +/- x 10 0 Tap here or pull up for additional resources LO 00Baking powder contains sodium bicarbonate plus an acidic salt like sodium acid tartrate or calcium acid phosphate. Suggest how baking powder can "raise" breads and pastries when mixed with water and heated.
- Complete and balance the precipitation reaction. Include physical states. Refer to the solubilities of common saltsas needed. CuCl2(aq) + Na2CO3(aq) -->Is it possible, upon precipitation of the third class ions, to add H2S first, then NH4OH and NH4Cl? And whyA volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?
- Please write the balanced chemical equations on the observations of heating NaHCO3 and bubbling the gas made by decomposition through the Ca(OH)2 solution in the presence of bromothymol (blue acid base indicator solution) Please write out in chemical equation form!Suppose you have a solution that might contain any or allof the following cations: Ni2+, Ag+, Sr2+, and Mn2+. Additionof HCl solution causes a precipitate to form. After filteringoff the precipitate, H2SO4 solution is added to the resultingsolution and another precipitate forms. This is filtered off,and a solution of NaOH is added to the resulting solution.No precipitate is observed. Which ions are present in each ofthe precipitates? Which of the four ions listed above must beabsent from the original solution?2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)