15. The pH of a solution of ferric nitrate, Fe(NO3)3, is not 7.00. This fact is...
The reaction between the compound [Fe (H2O).] (NO3)3 and Na (NSC) produces a red ferric thiocyanate complex, [Fe (H2O)-(NSC)] (NO3)2. Initial concentration of [Fe (H20)6] (NO3)3 and Na (NSC) were determined to be 0.025M and 0.050M. Equilibrium concentration of [Fe (H2O)s(NSC)] (NO3)2 was determined to be 0.016M. Calculate the equilibrium, Kc. [Fe (H20)6] (NO3)3 (aq) + Na (NSC) (aq) →[Fe (H,O)s(NSC)] (NO3)2 (aq) +NaNO3(aq) + H20(1)
The reaction between the compound [Fe (H2O).) (NO3)2 and Na (NSC) produces a red ferric thiocyanate complex, [Fe (H2O):(NSC)] (NO3)2. Initial concentration of [Fe (H2O).) (NO3)3 and Na (NSC) were determined to be 0.025M and 0.050M. Equilibrium concentration of [Fe (H2O)s(NSC)) (NO3)2 was determined to be 0.016M. Calculate the equilibrium, Kc. [Fe (H20).] (NO3)2 (aq) + Na (NSC) (aq) → [Fe (H2O):(NSC)] (NO3)2 (aq) +NaNO3(aq) + H20(1)
An aqueous solution of 0.40 M silver nitrate, AgNO3, and 0.40 M iron(II) nitrate, Fe(NO3)2, is allowed to reach equilibrium according to the following chemical reaction. Ag+(aq) + Fe2+(aq) equilibrium reaction arrow Fe3+(aq) + Ag(s) If the equilibrium constant, Kc, for the reaction is 1.7 at a certain temperature, determine the equilibrium concentrations of Ag+, Fe2+, and Fe3+.
The metathesis reaction between iron (III) nitrate and sodium sulfide is shown below 2 Fe(NO3)3(aq) + 3 Na2S (aq) ➝ 6 NaNO3(aq) + Fe2S3(s) How many grams of solid iron (III) sulfide can be produced by the reaction of 250.0 ml of 0.400 M iron (III) nitrate solution with 350.0 ml of 0.250 M sodium sulfide solution? Determine the final concentration of each ion in solution at the end of the precipitation reaction. Na+ NO3– Fe+3 S–2
Question 27 What is the hydronium ion concentration in a 0.5 M ammonia solution? (1 point) 3.0E11 M 3.1E-15 M 3.3E-10 M 3.3E-12 M Question 28 Identify the conjugate acid in the following reaction, HNO3(aq) + H2O() - NO3- (aq) + H3O+ (aq). (1 point) H20 H30+ NO3- None of the above Question 29
Question 10 10 pts Choose the correct, balanced chemical equation for the following neutralization reaction: nitric acid reacts with aqueous barium hydroxide to form aqueous barium nitrate and water HNO3 + BaOH - BaNO3 + H2O 2 HNO3(aq) + Ba(OH)2(aq) - Ba(NO3)2(aq) + 2 H20(1) HNO3(aq) + Ba(OH)2(aq) + Ba(NO3)2(aq) + H2O(1)
Calculating pH, POH, (OH) and (H30*] 2) A solution of HC2H302 has a concentration of 0.00045 M H what is the pH of the solution? (show your work). pH 3) If a solution has a concentration of 1.23x106 M H what is the concentration of OH? (show your work). rolul brenovadonismo loob [OH-] vor of 4) An unknown solution of HNO3(aq) has a pH of 2.96. What is the concentration of H (aq) in solution? (show your work). [H3O*) 9
The mole fraction of iron(III) nitrate, Fe(NO3)3, in an aqueous solution is 1.41×10-2. The percent by mass of iron(III) nitrate in the solution is -----%.
Calculate the molarity of Fe3+ in solution A. Solution A: 10 mL of 0.0600 M Fe(No3)3 + 15 mL DI water.
1. A 75.0-mL sample of 0.200 M Lead(II) nitrate, Pb(NO3)2, is reacted with 75.0 mL of 0.450 M KI solution and the following precipitation reaction occurs. Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) (a) Determine the limiting reactant. (b) How many grams of PbI2 will be formed if the yield is 100%? (c) What is the percent yield if 6.45 g of PbI2 were obtained? (2) K2Cr2O7(aq) + FeCl2(aq) → CrCl3(aq) + Fe(NO3)3(aq) (a) Determine the net ionic reactions and...