Pre-Laboratory Assignment Chemistry Hydrate Lab

Unformatted text preview: (53/3 Stoichiometry-Hydrates Prelaboratory Assignment Name and Drawer Number Q9 Q}: n I SCAN g‘fi ‘” £93 1. The data listed below was determined from the dehydration of the hydrate of magnesium sulfate. Mass of empty crucible = 35.794 g Mass of crucible and magnesium sulfate hydrate = 37.255 g Mass of crucible and anhydrous magnesium sulfate = 36.504 g 3. Write the chemical formulas for water and anhydrous magnesium sulfate. From the formulas calculate the molar masses of water and anhydrous magnesium sulfate. van-MU '23 \AarO ; Fiona 3imo‘ Our\\-“:§_\re'c$ \‘Ynsxnegwcm $‘0\\:O_5‘ Q— i\$ 1 at) o 5 l m0" b. Calculate the mass of water removed from the hydrate during the drying process from the difference between the mass of the crucible and hydrate and the mass of the crucible and the anhydrous salt. 0 a'\ ‘53\ E) be 0 3%“; guitalri‘wj / c. Use the mass of water (part lb) and the molar mass of water to calculate the moles of water in the sample. CncfiM-r W‘hu\ use (:1. Determine the mass of anhydrous magnesium sulfate by subtracting the mass of the empty crucible from the mass of the crucible containing the anhydrous compound. 0.110 5 /( e. Use the molar mass of the anhydrous compound and the mass of the anhydrous compound (part 1d) to determine the number of moles of anhydrous salt. ODOD%%$ mo\ M5504 f. Determine the ratio of the number of moles water in the hydrate to the number of moles of anhydrous salt in the hydrate by dividing the answer from part 1c by the answer from part 1c. This value is the number of moles of water in the hydrate for each mole of the anhydrous salt. Use this value to write the chemical formula for the hydrate. O I“ N W : 7.0a me" “BO/MM “as” 090°5%% chmvixgg} Qou W -41- "‘ Prelaborator)‘ Assignment - continued 2. A11 unknonn hydrated salt has the general formula Salt~nH20 where “n” is the number of moles of water for each mole of the hydrated compound. Although the chemical formula for the anhydrous salt is not known, it is known that the molar mass of the anhydrous salt is 151.92. The data listed below were obtained for a portion of the salt. (3) Determine the number of moles n of water in the hydrate for each mole of the anhydrous salt. (b) Write the formula for the salt, i.e., substitute the value of n into the general formula written above. Hint: It might be useful to follow the general solution outline used in question 1 of the Prelaboratory Assignment. Show the calculations. Mass of empty crucible = 35.107 g Mass of crucible and hydrated salt = 36.274 g Mass “crucible and anhydrous salt = 35.745 g _ “is “ (“Mafia Sn“ Ema. MA as.“ I c F - 3‘5. \0‘1 5 ml vaxix‘ow. ’ 0 .t; 35% so. \ - \\.o "t :5 \\\5qu¥: tux 93CL\¥- 3) mm of: \—\a0 \fi‘b\ N30: 3.x\.,00%-\\ + unmet: -(3 \q .Q:\\o % \XQD \\ (mask -»a\ A a o k 0 , muse 0'53 9&0 Mngb — O, oacvkwxcfiQsaG Ff, ‘ _ H \a \w'] S\\%d\ro}st¢3~ bc‘\¥ x \% ic\\o$ 9‘30 -W o .594; g) ‘R'axo f— so‘\1r -— O. QQQ‘AO ’mo\ 3Q\* O‘KPE’Q $30“ \:3\_O\';%SCLU¢ ® V&k\0 \e\ 0 0ean «WA 9‘30 A: "\ r“‘°_\______.—9‘ _—————r*""" mw-\ ww Ado - DO‘VBD “‘5‘ aflk , —42- 930A": ‘_l \'\ 9‘0 ...
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