According to the following reaction, what volume of 0.365 M Al(NO3)3 is needed to react with 30.0 mL of 1.07 M Na2CO3? 3 Na2CO3 (aq) + 2 Al(NO3)3 (aq) → 6 NaNO3 (aq) +Al2(CO3)3 (s) __________________ mL
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- According to the following reaction, what volume of 0.365 M Al(NO3)3 is needed to react with 30.0 mL of 1.07 M Na2CO3?
3 Na2CO3 (aq) + 2 Al(NO3)3 (aq) → 6 NaNO3 (aq) +Al2(CO3)3 (s)
__________________ mL
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- students are asked to prepare solid lead(II) chloride (PbCl2) according to the following balanced equation. if there is excess Pb(NO3)2 solution then how many grams of lead (II) chloride can be made from 100.0mL of a .425 M sodium chloride solution? Pb(NO3)2 (aq)+ 2NaCl (aq)= PbCl2 (s) +2NaNO3(aq)Calcium chloride and sodium hydroxide react according to the equation: CaCl2 (aq) + 2 NaOH (aq) → Ca(OH)2 (s) + 2 NaCl (aq) What volume of 2.00 M NaOH would be needed to react with 50.0 mL of 1.50 M CaCl2? (the answer is 75.0 mL, but I need to know how to get there)Na2CO3(aq) + CaCl2(aq) to 2NaCl(aq) + CaCO3(s) Calculate the volume (in mL) of 0.100 M CaCl2 needed to produce 1.00g of CaCO3(s) There is an excess of NaCO3 Molar mass of calcium carbonate = 100.09 g/mol Volume of calcium chloride = ________mL
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- Toxic cyanide ions can be removed from wastewater by adding hypochlorite. 2 CN−(aq) + 5 OCl−(aq) + H2O(?) → N2(g) + 2 HCO3−(aq) + 5 Cl−(aq) If 1.50 ✕ 103 L of 0.125 M OCl− is required to remove the CN− in 3.4 ✕ 106 L of wastewater, what is the CN− concentration in the water in mg/L? How many milliliters of 0.575 M AgNO3 would you need to add to a 50.00 mL aliquot of the final solution (consider the volumes simply additive) to precipitate the chloride ions formed in the reaction? Show work pleaseLead(II) nitrate and ammonium iodide react to form lead(II) iodide and ammonium nitrate according to the reaction Pb(NO3)2(aq)+2NH4I(aq)⟶PbI2(s)+2NH4NO3(aq) What volume of a 0.570 M NH4I solution is required to react with 445 mL of a 0.120 M Pb(NO3)2 solution? volume: mL How many moles of PbI2 are formed from this reaction? moles: mol PbI2Potassium hydroxide and iron(II) chloride combine in the precipitation reaction shown below. How many moles of iron(II) hydroxide can be produced in the reaction of 0.520 L of 3.4 M KOH with excess FeCl2? 2 KOH (aq) + FeCl2 (aq) ---> 2 KCl (aq) + Fe(OH)2 (s)
- In the reaction: 2NaOH(aq) + H2SO4(aq) → 2H2O(l) + Na2SO4(aq), what volume of 0.25 M NaOH would be needed to exactly react with 15 cm3 0.50 M H2SO4? Select one: a. 60 cm3 b. 15 cm3 c. 30 cm3 d. 7.5 cm31. What is the concentration, in parts per million, of a solution in which 600 grams of aluminum oxide, Al22O33, is dissolved in 2500 mL of solution?MM Al22O33- 101.96 g/mol.Express answer in 6 significant figures, without unit. 2. You have a stock 0.100 M solution of KMnO44 and I00-mL volumetric flasks. What volumes of the stock solution will you have to pipet into the flask to prepare a solution of 1.00 x 10−3−3 M KMnO44 solutions? Express answer in 3 significant figures, without unit. 3. Calculate the concentration of potassium sulfate in grams per liter if you have 0.250 M Potassium sulfate.Express answer in 3 significant figures, without unit.MM potassium sulfate is 174.25 g/mol . 4. How many possible constitutional isomers for C5H12C5H12? Type answer in numerical form.What is the concentration of sodium chloride in the final solution if 18.50 mL of 0.125 M BaCl2 completely reacts and the total volume of the reaction is 125.0 mL, given the reaction: BaCl2(sq) + Na2SO4(aq) --> BaSO4(s) + 2NaCl(aq) PLEASE USE THE CORRECT NUMBER OF SIGNIFICANT FIGURES
