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Fe3+(aq) + SCN-(aq) to Fe(SCN)2+(aq). Identify the reactant or product that increases or decreases when AqNO3 is added and AgSCN(s) formed.
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- Given the equation Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107 determine the concentration of NH3(aq) that is required to dissolve 669669 mg of AgCl(s) in 100.0 mL of solution. The KspKsp of AgCl is 1.77×10−101.77×10−10.1. What is the conjugate base of the formic acid HCO,H? 2. You have a 5.43 x 10 M solution of HNO, at 25 °C. Calculate the [OH] of this solution? 3. A solution that has a pH of 4.5 is (acidic, basic, neutral)? 4. A solution has a hydronium ion concentration of 3.2 x 10 M. Calculate the pOH.In the reaction Pb(s) + 2Ag1(aq) -----> Pb21(aq) + 2Ag(s) Which species is oxidized and which is reduced?
- Write the equilibrium constant expression for this reaction: CH₂OH(aq) + Cl(aq) → CH₂Cl(aq)+OH (aq) X 8 ŚIf Phenolphthalein was added to H2O (l) + CO2 (g) → H2CO3 (aq) what color would the solution be?Consider the titration of the weak acid, benzoic acid, HC7H5O2. Its acid dissociation reaction is: HC7H5O2 (aq) + H2O (l) ↔ C7H5O2- (aq) + H3O+ (aq) A 25.00 mL sample of a solution of benzoic acid, concentration unknown, is titrated with 0.0500M NaOH solution. A plot of the titration is shown below. 1. what is the pKa (approximately) of benzoic acid? Its Ka? 2. on the plot, indicate the buffering region of the titration 3. From the pH at the equivalence point, estimate the pKb of benzoate ion (conjugate base to benzoic acid)______________[Remember, at the equivalence point, C7H5O2- (aq) + H2O (l) ↔ HC7H5O2 (aq) + OH- (aq) ]
- A weak acid, HA, has a pKa = 6.2. If a solution of NaA(aq) is prepared, what does the pH of the solution need to be adjusted to in order to achieve the following ratios of deprotonated to protonated species? 1) [A-] / [HA] = 0.01 2) [A-] / [HA] = 10 3) [A-] / [HA] = 1 4) [A-] / [HA] = 106 Note: NaA is the sodium salt of , the conjugate base of HA. Assume NaA completely dissociates in water.Methyl orange is an indicator used for detecting the pH of acidic solutions. The red, protonated form of the indicator (HIn) dissociates into a yellow, deprotonated form (In¯) as shown in the reaction. The pKa for methyl orange is 3.4. HIn(aq) = H*(aq) + In¯(aq) yellow red Identify the color of a solution containing methyl orange Identify the color of a solution containing methyl orange indicator at pH 2. indicator at pH 3.4. orange yellow yellow orange red red Identify the color of a solution containing methyl orange indicator at pH 6. orange yellow redZn (s) + NO3- (aq) -> Zn2+ (aq) + NH3 (aq) Needs to be balanced in a basic solution
- Blood has a normal pH of about 7.40. Lactic acid has a pKa of 3.08. Is lactic acid predominantlyprotonated or deprotonated in blood?For the following, complete the equilibria, then state whether reactants or products are favored. Reactant Product Favored or not Favored a Fe(H2O)63+(aq) + OH2-(aq) ⇌ b H2SO3aq+ IO3-aq⇌ c CN-aq+ H2PO4-aq ⇌The amino acid alanine has two isomers, a-alanine and ẞ-alanine. When equal masses of these two compounds are dissolved in equal amounts of a solvent, the solution of a-alanine freezes at the lowest temperature. Which form has the larger equilibrium constant for ionization (HX=H+X-)? (A) B-alanine B a-alanine
