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Given that the Ksp for silver bromide is 3.3 x 10-13, which of the following solutions would NOT produce a precipitate of AgBr? and WHY?
(i) 0.20 M AgNO3 and 1.00 x 10-12 M CaBr2
(ii) 2.00 x 10-8 Ag2SO4 and 1.0 x 10-5 M NaBr
(iii) 0.20 M AgNO3 and 1.00 x 10-12 M NaBr
A. (i) and (ii)
B. (i) and (iii)
C. (ii) and (iii)
D. (iii) only
E. all three of (i), (ii), (iii)
Oxygen and sulfur combine to form a variety of differenet sulfur oxides. Some are stable molecules and some, including S2O2 and S2O3, decompose when they are heated
what will the final mixture contain if 14.0 g of N2 and 35.5 g of Cl2 react to completion and the balanced equation is: N2+3Cl2--->2NCl3
the partial pressures of gas A and gas B respectively are 0.298 ATM and .702 atm if 0.130 mol a 3rd gas is added with no change in volume or temperature, what would the total pressure become?
prepare 250ml of a .5 mol/L aqueous solution of magnesium nitrae, Mg(N3)2. what mass of magnesium nitrate do you need?
What would you expect to happen if an unknown solution that may contain ions from Groups I through IV were treated with Na2CO3 under basic conditions?
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A gas under a pressure of 74 mmHg and at a temperature of 75C occupies a 500.0-L container. How many moles of gas are in the container?
That would mean it wouldn't have any electrons to give. Can anyone answer this for me as to why there are 28 electrons being transferred if hydrogen has a oxidation state of +1 meaning it doesn't have any electrons to give?
The value for Ksp for manganese(II) hydroxide, Mn(OH)2, is 1.6 x 10^-13. Calculate the molar solubility of Mn(OH)2 in a solution that contains 0.020 M NaOH.
4 KO2 + 2 H2O + 4 CO2 4 KHCO3 + 3 O2 1.86 moles of O2 were produced.Now, How many molecules of O2 does this number of moles represent.
Calculate the pH at the equivalence point for the titration of 0.200 M methylamine (CH3NH2) with 0.200 M HCl.
Describe an expreiment to determine the molal freezing point depression constant
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