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A 0.2861 gram sample of an unknown acid (HX) required 32.63 mL of0.1045 M NaOH for neutralization to a phenolphthalein endpoint. Explain what is the molar mass of this acid? If this unknown acid had the formula H2X could this experiment be utilized to determine its molar mass? Explain why or why not.
how many ml of concentration sulfuric acid, 94%(g/100g solution), density 1.831 g/cm3 are required to prepare 1L of 0.100 M solution.
You have a solution made by dissolving 1.5230g of solid Na2(C2O4) and diluting to a volume of 250.00mL: How many moles of sodium ions are contained in this solution
Magnesium ions can be precipitated from seawater by the addition of sodium hydroxide. How much sodium hydroxide in grams must be added to a sample of seawater to completely precipitate the 82.0 mg of magnesium present
How many mL of 0.380 M solution can be prepared by dissolving 4.00g of Ca(OH)2 in water?
When 54.01 g of Ba(NO3)2 is dissolved into a total volume of 3.23L of solution.
An unknown gas sample was dissolved in water at 25°C, producing a solution with a concentration of 4.7 x 10-4 M at 522 mm Hg. What is the Henry's law constant for the unknown gas
To obtain a 18.0% (w/v) solution of copper sulfate (CuSO4), M.W = 160) when only the crystalline salt is available (CuSO4 x 5H2O, M.W. = 250) what should the crystalline salt be weight to prepare 450.0 mL of solution
Determine how long will it take for a sample of N2O5 to decay to sixty percent of its initial value?
Why is it an important concept that atoms generally appear in whole number molar ratios to each other in chemical compounds?
KCl and sucrose (C11H22O11) are desolved in the same beaker of distilled water. write one mass balance and one charge equation that describe the resulting solution
The initial DO of the mix is 9.0 mg/L. After 5 days, the DO is 4.0 mg/L. After a long period of time, the DO is 2.0 mg/L, and it no longer seems to be dropping. Assume nitrification has been inhibited so the only BOD being measured is carbonaceous..
What is the concentration ratio of CO2 (usually written as H2CO3) to HCO3- in blood at pH = 7.40. (carbonic acid Ka1 = 4.3 x 10-7)
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