A 130.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br.
A) What mass of HCl could this buffer neutralize before the pH fell below 9.00? answer to this was 0.088g
B) If the same volume of the buffer were 0.265 M in NH3 and 0.395 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?
In: Chemistry
A standard galvanic cell is constructed in which a Cd2+ | Cd half cell acts as the cathode. Which of the following statements are correct?
Hint: Refer to a table of standard reduction potentials.
(Choose all that apply.)
1. The anode compartment could be F2|F-.
2. The anode reaction could be Cr -> Cr3+ + 3e-
3. Cd2+ is reduced at the cathode.
4. As the cell runs, anions will migrate from the Cd2+|Cd compartment to the other compartment.
5. The cathode reaction is Cd -> Cd2+ + 2e-
In: Chemistry
In which of the following pairings of compounds are both members
of the pair strong
electrolytes?
| NaCN and LiI |
| NH3 and HI |
| NaOH and H2CO3 |
| KBr and HBr |
| more than one answer is correct |
In: Chemistry
In: Chemistry
draw full sn1 mechanism for a reaction that includes 2-methyl-2-propanol, n-pentanol and hydrochloric acid as the reactants and 2-chloro-2-methylbutane and 1-chloropentane as products.
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Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction
NH4HS(s)?NH3(g)+H2S(g)
This reaction has a Kp value of 0.120 at 25 ?C.
An empty 5.00-L flask is charged with 0.400g of pure H2S(g), at 25
?C.
What is the initial pressure of H2S(g) in the
flask?
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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
In: Chemistry
In: Chemistry
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)
In: Chemistry
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?
In: Chemistry
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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