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1) CaF2 at room temperature has a solubility of 0.00160 g of CaF2 per 100g of water. How many moles ofCaF2 are there?
2) If presuming a solution of CaF2 is saturated and has a density of 1.00g/ml; explain how many moles will dissolve in 1.00L of solution?
You are asked to determine the strength of an acid by titration with NaOH. Exactly 50.0 ml of the acid are titrated with 0.300M NaOH and the equivalence point is reached at exactly 20.0 ml of NaOH. What is the molar strength of the acid
A 14 mL sample of a solution of AlBr3 was diluted with water to 56 mL. A 25 mL sample of the dilute solution was found to contain 2.31 M Br-. What was the concentration of AlBr3 in the original undiluted solution
dinitrogen monoxide gas and 3.41g of carbon dioxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits..
a compound x contains the elements carbon hydrogen and oxygen. after 35 g of x were burned in pure oxygen 59 g of
suppose 4.00 mol of an ideal gas undergoes a reversible isothermal expansion from volume v1 to volume v2 6v1 at
A mixture of fuel containing 0.530 mol CH4/mol, 0.330 mol C3H8/mol, and 0.140 mol C5H12/mol at 60.0°C and 125 kPa (gauge) enters a furnace at a rate of 91.0 L/min where it reacts with 17.4% excess air.
You have standardized the NaOH solution that has a concentration of 0.05418 M. You are given a bottle of vineaga(acetic acid) with an unknown concentration.
During a breath, the average human lung expands by about 0.50L. If this expansion occurs against an external pressure of 1.0 atm, how much work in J is done during the expansion?
Perform the following mathematical operations, and express each result to the correct number of significant figures. 0.19*6.022*10^23
A compound contains the following: 84.1% C and 15.9% H. The molecular mass of the compound is 120 g/mol. What is the empirical formula and molecular formula
Calculate the heat released as 115 grams of water cool from its normal boiling point (100 degrees C) to a temperature of 33 degrees C.
The mass of a beaker is 5.333 g. After 5.00 mL of a concentrated hydrochloric acid solution is pipetted into the beaker, the combined mass of the beaker and the hydrochloric acid sample is 11.229 g. From the data, what is the measured density of t..
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