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A 20.0 mL sample of hypobromous acid (HBrO) was titrated with 0.180 M KOH. To reach the equivalence point required 27.75 mL of KOH. Ka for HBrO is 2.8 x 10^-9
a) what is the initail pH of this solution of hypobromous acid?
b) what is the pH of the solution at the equivalence point?
c) what would the pH of the solution be after the addition of the first 10.00 mL of base?
d) What would be the pH after adding 30.0 mL of the base?
the mass natural abundance of the isotopes h and d are 99.985 and 0.015 respectively. the mass natural abundance of
0.2 m hcl is used to neutralize 20 ml of 0.35 m naoh.a.how many moles of oh- are present?b.how many moles of h are
When dealing with ICE tables and calculating Kb and such, how do you do the algebra to calculate x when x is NOT negligible?
A solution of 120 mL of 0.150 M KOH is mixed with a solution of 280 mL of 0.250 M NiSO4. How many grams of the precipitate can be formed?
Each reaction needs to be balanced and all physical states (s, l, g, aq) noted (you may need to look these up or read the lab to determine the physical states).
Calculate the value of the solubility product constant for PbSO4 from the half-cell potentials. PbSO4(s) + 2e- ? Pb(s) + SO42-(aq) Eº = (-0.383) V Pb2+ + 2e- ? Pb(s) Eº = (-0.127) V These half-cell potentials are not accurate.
calculate the minimum energy a photon must have to produce an electron hole pair in an extrinsic semiconductor of band gap 1.3 electron volts.
radioactive isotope x has been found in rock units s and q. isotope x breaks down into isotope z with a half life of
A titration of 200.0 mL of 1.00 M H2A was done with 1.28 M NaOH. For the diprotic acid H2A, ka1 = 2.5 x 10^-5 and ka2 = 3.1 x 10^-9.
Assuming gasoline is 89.0% isooctane, with a density of 0.692 g/mL, what is the theoretical yield (in grams) of CO2 produced by the combustion of 1.56 x 1010 gallons of gasoline
If the initial pressure of NH3(g) is 1.766 atm, calculate the % of NH3(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kp at 600.0 °C is 455000.00. The initial pressure of the reaction products ..
The equilibrium constant K(p) for the reaction: H2(g)+I2(g)-> 2HI(g) at this temperature is 54.3. Determine the equilibrium partial pressures of H2, I2, and HI
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