Write the Ksp expression.
Substitute 0.0050 for (Fe^3+) and solve for (OH^-).
A is a solution of trioxonitrate(v) acid, HNO3, of unknown concentration. B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25cm3 portions solution B required an average of 24.00cm3 of solution A for neutralization, using
4. At high temperatures, nitrogen dioxide, NO2, decomposes into NO and O2. If y(t) is the concentration of NO2 (in moles per liter), then at 600 degrees K, y(t) changes according to the reaction law dy/dt = −. 05y2 for time t in seconds. A. Express y in
The initial concentration of a reactant in a first order reaction is 0.620 molar. What will be its concentration after 3 half-lives? I did 0.620 -> 0.31 ->0.155 0.155M will be the concentration. Is this correct?
For the equilibrium H2(g)+CO2(g)H2O(g)+CO(g) Kc=3.18 at 1106 K.If each of the four species was initially present at a concentration of 3.000M,Calculate the equilibrium concentration of the CO (g) at this temperature. Choices 0.844 3.268 3.844 3.460 2.156
What is the concentration of the Mg2 ion in solution when [CO3-2] = 0.25M given that the Ksp= 6.82 x 10-6 for the following reaction MgCO3-------->Mg +. CO32- Chemistry - DrBob222, Friday, November 11, 2011 at 5:34pm Ksp = (Mg^2+)(CO3^2-) Substitute 0.25M
Calculate the concentration of all species in a 0.145 M solution of H2CO3 (Ka1 is 4.3×10−7 and Ka2 is 5.6×10−11). Calculate the concentration of H2CO3. Calculate the concentration of HCO−3. Calculate the concentration of CO2−3. Calculate the
When 10.0 mL of 0.012 M Pb(No3)2 is mixed with 10.0 mL of 0.030M KI, a yellow precipitate of PbI2(s) forms. a. Calculate the molarity of [Pb2+] b. calculate the initial molarity of [I-] c. On measuring the equilibrium concentration of [I-] it cam out to be
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca^2+ (aq) and 0.0390 M Ag^+ (aq). What will be the concentration of Ca^2+ (aq) when Ag2SO4(s) begins to precipitate? What percentage of the Ca^2+ (aq) can be separated from the Ag^+ (aq) by
At 22 °C an excess amount of a generic metal hydroxide M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.56. What is the Ksp of the compound at 22 °C? I have found my [OH-] concentration (3.63x10^-4) but I'm not sure I'm
Calculate the solubility of AgCl in: Ksp = 1.6x10^-10 a) 100 ml of 4.00 x 10^-3 M Calcium chloride b) 100 ml of 4.00 x 10^-3 M Calcium Nitrate all i know is 1.6x10^-10=[Ag+][Cl-] which is 1.6x10^-10=x^2 x=1.3x10^-5, giving the M of Ag and Cl. Don't know
You can ask a new question or browse existing questions.