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A 0.3146-g sample of a mixture of NaCl(s) and KBr(s) was dissolved in water. The resulting solution required 51.30 mL of 0.08765 M AgNO3(aq) to precipitate the Cl-(aq) and Br-(aq) as AgCl(s) and AgBr(s). Calculate the mass percentage of NaCl(s) in the mixture.
What volume of 0.2500 M cobalt(III) sulfate is required to react completely with a) 25.00 mL of 0.0315 M calcium hydroxide?
What is the molecular geometry around a central atom that is sp3 hybridized and has one lone electron-pair? a.bent, b. linear, c.trigonal-planar
Analysis shows that there are 1.8 moles of H2, 7.45e-05 moles of S2, and 7.2 moles of H2S present in a 50.8 L flask at equilibrium. Calculate the equilibrium constant Kc for the reaction.
What is the molar solubility of Hg2C2O4 (Ksp = 1.75x10^-13) in 0.34M Hg2(NO3)2
calculate the atomic mass of an element with a measure specific heat of 0.14 J/(g C). Express your answer in atomic mass units to two significant figures.
suppose a student attempts to do an ion exchange on a column that is already nearly saturated with CO2+ and Zn2+.
What is the mass of a rectangular piece of copper 24.4cm x 11.4cm x 6.6cm? The density of copper is 8.92 g/cm^3.
determines how many grams of glucose are in 100 mL of the final solution?
How many grams of NO(g) can be formed from 3.0 moles of NH3(g) if there is sufficient O2(g) to use all of the ammonia?
N2(g) + 3H2 (g) ---- 2NH3(g) a one liter vessel contain 1.60 mole NH3.800 mole N2 and 1.20 mole of H2. What is the equilibrium constant.
A 49 gram sample of impure potassium nitrate (KNO3) was heated to complete decomposition according to the equation 2 KNO3(s) → 2 KNO2(s) + O2(g) After the reaction was complete.
A student wants to prepare a dilute solution of iron (III) solution, . The student is provided with a stock solution of 0.800 +/- 0.001 M and a 100.00 +/- 0.008 mL volume trick flask since the experiment trquires about 80 mL of the dilute iron (II..
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