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A 250 mL stock solution contains 2.3 M Ca(CN)2. When 100 mL of the stock solution is diluted to 125 mL, how many moles of CN- ions will be contained in the dilute solution?
In an experiment for measuring water hardness in a water sample, using Atomic Absorption Spectrophotometry, I obtained a value of 173.74 ppm hardness for my water sample.
if molarity of a 2000ml solution is 4.0M NaCl, how many moles of NaCl are dissolved in that solution.
54.0 mL of a 1.40 M solution is diluted to a volume of 218 mL. A 109-mL portion of that solution is diluted using 183 mL of water. What is the final concentration.
Two scientists are experimenting with pure samples of isotope X, a highly radioactive substance. The first scientist has a sample with a mass of 20 grams.
The concentrations of lead in blood samples are often reported in units of micromoles of lead per liter of blood. Calculate the value of the concentration in these units of a blood sample containing 45 ppb lead.
What happened when 6.0M HCl was added to the contents of the tube in 7a above?
Determine its molecular formula if the molar mass of the compound = 199.55 grams per mole?
Describe how this observation is consistent with the law of conservation of charge.
The substance CS2 has a melting point of -110.8°C and a boiling point of 46.3°C. Its density at 20°C is 1.26 g / cm3. It is highly inflammable. a.)Name this compound.
A 1.17 g sample of an alkane hydrocarbon gas occupies a volume of 674 mL at 28°C and 741 mmHg. Alkanes are known to have the general formula CnH2n+2.
Consider an experimental run at 273 rm K where the initial number of moles (n_1) is actually 1.00 rm mol, and the final number of moles (n_2) is 2.00 rm mol.
Calculate the molar concentration of OH - ions in an 1.43 M solution of hypobromite ion, BrO- (Kb = 4.0 10-6).
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