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- Given the following data for the hydrate M(NO3)3 dot X H2O, where M is a metal with the atomic mass 90.97 g/mol, Mass of Crucible and Lid 34.0386 Mass of Crucible, Lid and Hydrate 39.4586 Mass of Crucible, Lid and Anhydrous Salt (3rd Heating) 37.3780 What was the mass percent of water in the hydrated salt, with the correct significant figures? Express units as %If 31.0 g of MgSO4⋅7H2O is thoroughly heated, what mass of anhydrous magnesium sulfate will remain? Express your answer to three significant figures and include the appropriate units.Given: Weight of silver chloride: 0.750g MW of silver nitrate: 170 g/mol MW of silver chloride: 143 g/mol mEq of silver nitrate: 0.170 Normality of silver nitrate: 0.105 N Unknown: Volume of Silver nitrate How much (mL) silver nitrate is required for the standardization? a. 4.995 b. 49.950 c. 49.590 d. 45.990
- If 10.00 ml of 0.0131 M KIO3 are used in the first part of the standardization process, how many moles of KIO3 are present?(Your answer should have 3 sig figs)(Recall that answers in scientific notation are entered as 1.234 E-5 for example)Cobalt(II) chloride forms several hydrates with the general formula CoCl2·xH2O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure CoCl2 behind. Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 22.%. Which hydrate is it? That is, what is x?Imagine that you are given 0.2500 g of a sample of copper(II) sulfate pentahydrate (CuSO4 • 5 H2O). You very carefully heat the compound for an extended period of time to drive off water, after which you determine the mass of the remaining solid to be 0.1598 g. Determine whether the data given confirm the formula of the hydrate. You must show any relevant calculation
- Cobalt(II) chloride forms several hydrates with the general formula CoCl2 ·x H2O , where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure CoCl2 behind. Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 22.% . Which hydrate is it? That is, what is x ?320.4 grams of isomaltitol, C12H24O11, was combusted in a furnace completely in an excess oxygen. The products of this reaction are liquid water and gaseous carbon dioxide. How much water (in kg) do you expect from this reaction assuming that all of the isomaltitol reacts? Enter your numeric answer in the units of kg. Do not enter the unit. Use enough significant digits to prevent rounding errors. Hint: balance the reaction first. Recall that 1 kg = 1000 g.(NH4)2Cr2O7 (s) -------> Cr2O3 (s) + 4 H2O (g) + N2 (g) calculate the number of grams of chromium(III) oxide, Cr2O3, would be formed if 10.00 grams of ammonium dichromate, (NH4)2Cr2O7, were used in the reaction. Place the answer in the box below and be sure to report the answer using the correct number of significant digits and place the unit "g" after the numerical answer. (Note: MM of (NH4)2Cr2O7 = 252.10 g/mole; MM of Cr2O3 = 152.00 g/mole)
- The sulfur in an 3-tablet shape of captodiamine C21H29NS2 was converted to sulfate and determined gravimetrically. Calculate the average mass (in mg) of captodiamine per tablet if 0.679 g of barium sulfate was recovered.Determination of the amount of water, mass of crucible + dehydrated sample 16.2265g, mass of dehydrated Sample is 1.3031g, mass of water is 0.3587g, moles of water is 0.01991moles,DETERMINATION of the amount of copper, mass of copper 0.6291g, moles of copper 9.900 × 10 to the negative 3 moles, Determination of the amount of chlorine, calculate mass of copper + water.The following ratios of NaOH to HCl were determined in an analysis: T1 = 0.9958, T2 = 0.9929. How much is the precision?