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In: Chemistry
A 50.0 ml sample of 0.00200M AgNO3 is added to 50.0 ml of 0.00100M NaIO3. What...
A 50.0 ml sample of 0.00200M AgNO3 is added to 50.0 ml of 0.00100M NaIO3. What is the equilibrium consentration of Ag+ in solution? (Ksp for AgIO3 3.0 x 10 -8) Answer is 7.5 x 10 -6
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
A 50.0 mL sample of 0.0645 M AgNO3(aq) is added to 50.0 mL of 0.100 M...
A 50.0 mL sample of 0.0645 M AgNO3(aq) is added to 50.0 mL of
0.100 M NaIO3(aq). Calculate the [Ag+] at equilibrium in the
resulting solution. The Ksp value for AgIO3(s) is 3.17 × 10-8.
[Ag+] =____ mol/L
50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of 0.050 M NaCl. Calculate...
50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of
0.050 M NaCl. Calculate the concentration of Ag + and Cl- in the
resulting solution, assuming the volumes are additive.
Ksp(AgCl) = 1.82*10-10
if 30.0 ml of 0.150M CaCL2 is added to 15 ml of 0.100M AgNO3. what is...
if 30.0 ml of 0.150M CaCL2 is added to 15 ml of 0.100M
AgNO3. what is the mass in grams of AgCL precipitate?
When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH,...
When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH,
the temperature change was 5.8 *C. Calculate the heat change for
the reaction (Qsoln) and the heat of neutralization
(ChangeHneut), and the state whether the reaction is
exothermic or endothermic.
When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH,...
When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH,
the temperature change was 5.8 *C. Calculate the heat change for
the reaction (Qsoln) and the heat of neutralization
(ChangeHneut), and the state whether the reaction is
exothermic or endothermic.
1a )When 50.0 mL of 0.500 M HCl at 25.0°C is added to 50.0 mL of...
1a )When 50.0 mL of 0.500 M HCl at 25.0°C is added to 50.0 mL of
0.500 M NaOH at 25.0°C in a coffee cup calorimeter, the temperature
of the mixture rises to 28.2°C. What is the enthalpy of reaction
per mole of acid? Assume the mixture has a specific heat capacity
of 4.18 J/(g ? K) and that the densities of the reactant solutions
are both 1.00 g/mL.
1b) Consider the following reaction: 2 PbS (s) + 3 O2...
In a constant-pressure calorimeter, 50.0 mL of 0.330 M Ba(OH)2 was added to 50.0 mL of...
In a constant-pressure calorimeter, 50.0 mL of 0.330 M Ba(OH)2
was added to 50.0 mL of 0.660 M HCl. The reaction caused the
temperature of the solution to rise from 21.85 °C to 26.35 °C. what
is ΔH for this reaction (KJ released per mole of H2O produced)?
Assume that the total volume is the sum of the individual volumes
and that the density and heat capacity are equal to that of
water.
In a constant‑pressure calorimeter, 50.0 mL 50.0 mL of 0.800 M H2SO40.800 M H2SO4 was added...
In a constant‑pressure calorimeter, 50.0 mL 50.0 mL of 0.800 M
H2SO40.800 M H2SO4 was added to 50.0 mL50.0 mL of 0.370 M
NaOH.0.370 M NaOH.
The reaction caused the temperature of the solution to rise from
23.40 ∘C23.40 ∘C to 25.92 ∘C.25.92 ∘C. If the solution has the same
density and specific heat as water (1.00 g/mL1.00 g/mL and 4.184
J/(g⋅°C),4.184 J/(g⋅°C), respectively), what is Δ?ΔH for this
reaction (per mole of H2OH2O produced)?
Assume that the total volume...
When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF,...
When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M
NaF, CaF2 precipitates, as
shown in the net ionic equation below. The initial temperature of
both solutions is 25.00°C. Assuming
that the reaction goes to completion, and that the resulting
solution has a mass of 100.00 g and a heat
capacity the same as water, calculate the final temperature of the
solution.
Ca2+(aq) + 2 F-(aq) → CaF2(s)
ΔH° = –11.5 kJ
When trying to...
When 50.0 mL of 0.900 M Ca(NO3)2 is added to 50.0 mL of 1.80 M NaF,...
When 50.0 mL of 0.900 M Ca(NO3)2 is added to 50.0 mL of 1.80 M
NaF, CaF2 precipitates, as shown in the net ionic equation below.
The initial temperature of both solutions is 30.00°C. As the
reaction proceeds, the temperature rises to 31.50 °C. Assuming that
the reaction goes to completion, and that the resulting solution
has a mass of 100.0 g and a specific heat of 4.18 J/(g ∙ °C),
calculate the ΔH° for this reaction, expressed in kJ/mol...
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