A 50.0 mL sample of 0.0639 M AgNO3(aq) is added to 50.0 mL of 0.100 M...
Kererences CHEMWORK A 50.0 mL sample of 0.0495 MAgNO3(aq) is added to 50.0 mL of 0.100 M NaIO3(aq). Calculate the [Ag ] at equilibrium in the resulting solution. The Kap value for AgIO3(s) is 3.17 x 10-8 [Ag']=| mol/L Submit Chow Hints
A 50.0-mL sample of 0.00200 M AgNO3 is added to 50.0 mL of 0.0100 MNalo3. What is the equilibrium concentration of Ag in solution? (Ksp for Ado3 is 3.0 x 10-8.) Concentration mol/L
50.0 mL of 0.100 mol/L HCI is added to 50.0 mL of 1.00 mol/L NaOH Calculate the hydronium and hydroxide concentrations o f the resulting solution. Explain.
Suppose that 51.0 mL of 0.11 M AgNO3 is added to 50.0 mL of 0.048 M NaCl solution. (a) What mass of AgCl will form? g AgCl the tolerance is +/-2% (b) Calculate the final concentrations of all of the ions in the solution that is in contact with the precipitate. [Ag+] = × 10 M [NO3−] = × 10 M [Na+] = × 10 M [Cl−] = × 10 M (c) What percentage of the Ag+ ions have precipitated?...
Calculate the equilibrium concentration of Ag+(aq) after 10.0 mL of 0.100 M AgNO3(aq) have been mixed with 10.0 mL of 1.00 M NaCN(aq).
help please! 4. You added 0.05 mL of 0.10 M AGNO3 to 4.0 mL of 2.0 M NaCl, and formed a saturated solution of AgCl (s): K=Ksp Ag (aq)+ CI (aq) AgCl (s) Using this saturated solution as the test solution you set up the following cell AglAg' (test solution after reaction)||Ag* (1.0M) |Ag and measured Ecell= 0.61 V. (a) Using the measured value of Eel and Eq (15), calculate the equilibrium [Ag'] (i.e. of the test solution after reaction)....
In a coffee-cup calorimeter, 50.0 ml of .100 M AgNO3 and 50.0 ml of .100 M HCl are mixed to yield the following reaction: Ag+(aq) + Cl-(aq) --> AgCl(s) The two solutions were initially at 22.6°C and the final temp is 23.4°C. Assume that the final solution has a mass of 10.0 g and has a specific heat capacity of 4.184 J/g°C. Calculate delta for the reaction in kJ/mole of AgCl formed.
If 37.5 mL of 0.100 M NaOH is added to 10.0 mL of 0.100 M CH3COOH, what will be the pH of the resulting solution? CH3COOH(aq)+OH−(aq)→CH3CO−2(aq)+H2O(l)
50.0 mL of a 0.250 M AgNO3 solution and 50.0 mL of 0.400 M Na2CO3 solution are mixed. How much of the silver carbonate precipitate will be formed? 2 AgNO3 (aq) + Na2CO3 (aq) -> Ag2CO3 (s) + 2 NaNO3 (aq)
To determine the solubility product, Ksp, for Ag2CO3, 1.00 mL of 1.00 mol/L Na2CO3(aq) and 1.00 mL of 0.100 mol/L AgNO3(aq) were combined. The mixture was stirred for 10 minutes to ensure that equilibrium had been reached. A voltaic cell was constructed to determine the concentration of soluble Ag (aq) ions left in solution at equilibrium, and [Ag leg was thus found to be 2.0 x 10-7 mol/L. Calculate the equilibrium concentration of CO32-(aq) ions left in solution at equilibrium,...