Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa. Ka (HCOOH) = 1.7x10-4 ? 3.4% is correct answer
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Calculate the pH at the equivalence point in titrating 0.110 M solutions of each of the following with 8.0×10−2 MNaOH. chlorous acid (HClO2) benzoic acid (C6H5COOH)
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For each reaction listed, determine its standard cell potential (in V) at 25°C and whether the reaction is spontaneous at standard conditions.
(a) 2 Au(s) + 3 Zn2+(aq) → 2 Au3+(aq) + 3 Zn(s)
(b) Co2+(aq) + Hg(l) → Co(s) + Hg2+(aq)
(c) Cu(s) + Fe(NO3)3(aq) → CuNO3(aq) + Fe(NO3)2(aq)
(d) Sn(NO3)2(aq) + Zn(s) → Sn(s) + Zn(NO3)2(aq)
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A(aq) + B(aq) → 2C(aq)
If Kc = 3.4 x 10-17, this indicates that .....
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At equilibrium there will be nearly equal amounts of reactant and product. |
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At equilibrium there will be no product formed. |
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At equilibrium there will be considerably more product than reactant. |
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At equilibrium there will be considerably more reactant than product. Which of the following are true for all reactions that have achieved equilibrium?
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What mass of sucrose (C12H22O11) should be combined with 485 g of water to make a solution with an osmotic pressure of 8.00 atm at 280 K ? (Assume the density of the solution to be equal to the density of the solvent.)
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Give one advantage and one disadvantage of using a plasma excitation source (as oppaosed to a flame) for emission spectroscopy.
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A student reacts 96g of salicylic acid with 10 mL of acetic anhydride producing 10.7g of acetyl salicylic acid. What is the percent yield of the reaction?
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A system initially contains 2 lb of liquid water at 110ºF and 0.4 lb of ice at 32 ºF. The system attains an equilibrium state, while pressure remains constant at 1 atm. For water, the specific enthalpy change for a phase change from solid to liquid at 1 atm is 144 Btu/lb. If heat transfer with the surroundings is negligible, determine
(a) the final temperature, in ºF
(b) the amount of entropy produced in the process, in Btu/ºR.
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1. Explain how steps in a procedure remove impurities
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Which of the following substances has the lowest boiling point? C12H16 CH2Br2 Br2 ICl
How much energy in kJ will it take to melt 5.0 g of frozen Ar at -190o C?
T/F if methane was at -50o C it cannot be made to liquify at any pressure.
If H2O at -1.0o C and 1.0 atm has enough pressure applied to it, what phase change, if any, can occur?
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solid to liquid |
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liquid to solid |
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stays solid |
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stays liquid What is the concentration in percent by mass when a solution is prepared by dissolving 8.00 g of NaCl into 70.0 g of water? What kind of solute gets more soluble as the temperature of the solvent decreases? The normal vapor pressure of water at 30o C is 31.82 mmHg. When 25.0 g of glucose (C6H12O6) are dissolved in 25.0 g of water at 30o C, what is the solution's vapor pressure? What is the freezing point of a solution made up of 150.0 g of benzene (normal fp=5.5o C, Kf=5.12 oC/m) with 0.200 moles of naphthalene dissolved in them? |
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Consider the following reaction between oxides of nitrogen: NO2(g)+N2O(g)?3NO(g)
1.
Calculate ?G? at 800 K, assuming that ?H? and ?S? do not change with temperature.
Express your answer using two significant figures.
2.Calculate ?G? at 1000 K.
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If a solution containing 45 g of mercury(II) nitrate is allowed to react completely with a solution containing 14.334 g of sodium sulfate. a)How many grams of solid precipitate will be formed? b)How many grams of the reactant in excess will remain after the reaction?
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Consider a 0.5 M solution of trimethylammonium chloride. The ion trimethylammonium is the conjugate acid of the the weak base trimethylamine.The pKb of trimethylamine is 4.2
A) Calculate [H+]
B) calculate the concentration of trimethylammonium ions
C) calculate the concentration of trimethylamine in equilibrium
D) calculate [OH-]
E) Calculate [Cl-]
F) Calculate the pH
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