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1. Assume that the smallest volume that youcan dispense is 1.0 ml and that you have 3.5 L of an inexpensivediluent. You have a stock solution that has a concentration of8 M, and you need to make 100 ml of the final 0.4 nM working solution.
2. How would you make a 5 M solution of a substance with a molecular weight of 45 g/mol?
3. How would you make 1 mL of an 5 M solution? 1 μL?
Calculate the concentration of the dye in solution C in units of moles per Liter Kool Aid Solution, i have a molar absorptivity of 2.41x10^4 L/mol-cm analytical wavelength of 505nm molecular weight of 496.42g/mol, absorbance of 1.528
Write the balanced formula unit equation for the reaction of tetraphosphorus decoxide, P4O10, with water to form an acid
Milk of magnesia, Mg(OH)2, is prepared from aqueous solutions of magnesium sulfate and sodium hydroxide. If a solution containing 50.0g of MgSO4 is added to a solution with 50.0g of NaOH, what is the limiting reactant and mass of milk of magnesia ..
An evaluation of R was performed, following the procedure described in this module. The barometric pressure was 736 torr, the temperature was 295k and volume of hydrogen gas collected was 35.6 mL. The calculated value of R was 82.1 mL atm K^-1 mol..
The ΔGo for the change from liquid to gaseous water is positive. non-spontaneous. However, we all know that liquid water evaporates easily.
if 19.65mL of .145M nitric acid is required ti neutralize 50.0mL of barium hydroxide what is the molar concentration of the base? 2HNO3+Ba(OH)2-->Ba(NO3)2+2H2O
What volumes of the stock solution will you have to pipet into the flasks to prepare standards of 1.00, 2.00, 5.00 and 10 x 10 -3 M KMnO4 solutions?
the amount of product (3.80 mol P2O5) formed from the given amount of phosphorus and excess oxygen. In Part B, you found the amount of product (3.40 mol P2O5) formed from the given amount of oxygen and excess phosphorus.
An unknown element, X, reacts with sulfur to form an ionic compound having the empirical formula (S is sulfur). If the ion X has 21 electrons, identify the element
For which of the following general classes of compound do the member NOT exhibit a common structural feature or function
1.56 g of a gas dissolves in 2.00 L of water at a pressure of 1.75 atm. At what pressure will 2.00 g of the gas dissolve in 2.00 L of water if the temperature remains constant?
If the final tempurature of the combined water is 42.0 degrees C and the heat capacity of the calorimeter is 26.3 J/degrees C , calculate the mass of the water originally in the calorimeter
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