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A saturated solution of calcium iodate, Ca(IO3)2, is created by suspending a small amount of pure solid of Ca(IO3)2 in 50.0 mL of distilled water. After allowing equilibrium to be established, a 10.0-mL sample of the saturated solution is pipeted into an Erlenmeyer flask, and about 20 mL of de-ionized water is added to this sample, followed by about 1 cm3 of solid KI and 1 mL of 2.0 M HCl. The addition of excess KI and HCl converts all of the IO3- present in the sample to molecular iodine according to the following equation. IO3-(aq) + 5 I-(aq) + 6H+(aq) ? 3 I2(aq) + 3H2O(l) (Eqn-1) The iodine produced by the above reaction is then titrated with 0.0250 M Na2S2O3 using starch indicator, which requires 29.0 mL of 0.0250 M Na2S2O3 to reach end-point. The stoichiometric reaction between iodine and thiosulfate is represented by the following net ionic equation. I2(aq) + 2 S2O32-(aq) ? 2 I-(aq) + S4O62-(aq) (Eqn-2) Using Eqn-1 and Eqn-2, write a balanced net ionic equation that shows the stoichiometric relationship between iodate, IO3- and the thiosulfate, S2O32-, in acidic solution. (b) Use the equation derived from (a) and the data gi
A gas expands and does P-V work on the surroundings equal to 321 J. At the same time, it absorbs 177 J of heat from the surroundings. Calculate the change in energy of the gas.
Calculate the numbers of moles of 2-butanol that needed to dissolved in ethenol(125gms) just to form 12 m 2 butanol soln also find out mass of 2-butanol ?
How much KClO3 in grams is needed to generate 7.50L of O2 at pressure of 1.00atm and temp of 298K?
Express the concentration of a 0.0720 M aqueous solution of fluoride, F-, in mass percentage and in parts per million
If iron is oxidized to Fe2+ by a copper(II) sulfate solution, and 0.538 grams of iron and 13.0 mL of 0.40M copper(II) sulfate react to form as much product as possible.
CaCO3(s) + 2 HCl(aq) -> CaCl2(aq) + H2O(l) + CO2(g) How many mol CaCO3 can be dissolved in 0.0575 mol HCl?
Calculate the enthalpy of the reaction: 2NO(g) + O2(g) --> 2NO2(g) given the following reactions and enthalpies of formation: 1/2 N2(g) + O2(g) --> NO2(g), delta H *A = 33.2 kJ 1/2 N2(g) + 1/2O2(g) --> NO(g), delta H *B= 90.2 kJ
the osmotic pressure of the solution is 0.443 atm. What is the percent ionization of this acid? I got 20% but its wrong
A solution is prepared by adding 1.10 g of solid NaCl to 50.0 mL of 0.100 M CaCl_2. What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.
refer to the given equation as 4NH3(g) + 7O2(g) = 4NO2(g) + 6H2O(g) How many moles of ammonia will be required to produce 13.8 mol of water.
a 35.00 mL sample of NaOH solution is titrated to an endpoint by 14.76 mL of 0.4122M HBr solution, what is the molarity of the NaOH?
The first-order decomposition of phosphene to phosphorus and hydrogen 4PH3(g) → P4(g) + 6H2(g)
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