manual

What is the value in the concentration of the SCN Suppose the Keq for this experiment is 523. The initial concentration of the Fe+ is 4.00 x 10-2 M The initial concentration of the SCN is 1.00 x 10-3 M The reaction of the experiment: Fe3++ SCN 2 Fe(NCS)2+ The concentration of the SCN at equilibrium is : Y x 104M Your answer should have 2 sf

There are several chemical equilibria taking place in a solution of carbon dioxide in water: 1. CO₂(g) + CO₂(aq) 2. CO₂(aq) + H₂O(l) = H₂CO3(aq) 3. H₂CO3(aq) HCO3(aq) + H+ (aq) 4. HCO3(aq) = CO3²-(aq) + H*(aq) If OH- (from a strong base such as sodium hydroxide) is added to a solution of carbon dioxide, what happens to the OH- and what effect will this have on the equilibria above? Select one: OH-(aq) reacts with the H*(aq) ions to form water (which is only very slightly dissociated). This shifts the third and fourth reactions to the right. However, there is no H*(aq) involved in either the first or second reactions, so these equilibria will remain unaffected by the additon of OH¯(aq). O OH-(aq) is not involved in any of the four equilibrium reactions that carbon dioxide participates in and so the OH-(aq) will have no influence on the carbon dioxide equilibria Carbon dioxide dissolves and then reacts to produce the acidic carbonic acid molecule (H₂CO3). The H₂CO3 molecule is only…

Write the basic equilibrium equation for (CH3)2NH. Be sure to include the proper phases for all species within the reaction. 1 U + 4 2 0₂ Reset ( H₂O 3 ) 4 5 → (CH3)2NH OH- 5 6 6 (s) 2+ 7 N H3O+ 3+ 4+ 8 9 0 ☐o (1) • H₂O 9 (g)) (aq) H Delete

Try Again Check your exponents. Write the concentration equilibrium constant expression for this reaction. 3 1₂(s) + 2 Cr³+ (aq) + 7 H₂O(1)→ Cr₂O² (aq) +61¯ (aq) + 14 H* (aq) [₂0][₁][H]¹⁹ 3+ [¹] Η + 19 X Ś 00

The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20.  Suppose a chemist mixed 33.23 mg of Mg2+(aq)  with 44.56 mg of AsO43-(aq) in 21.47 Liter of water.  Which way will the equilibrium shift? Question 10 options:   right   left then right   left   at equilibrium then right    at equilibrium then left   not enough information   at equilibrium       right then left   can't be determined

2 An equilibrium constant describes the ratio of products over reactants in a particular situation. In this experiment, the equilibrium constant represents the balance between the yellow and blue forms of Bromothymol Blue. These colors are dependent upon the pH of the solution, Summarize how the design of this experiment relates the absorbance values of the yellow and blue version of the dye Bromothymol Blue to their respective concentrations.

Write the equation for the equilibrium constant (K) of the reaction studied in this exercise. 2CrO4 2- (aq) + 2H+ (aq) = Cr₂O72- (aq) + H₂O(1) 1E T² B 1 U T₂ 0 Word(s)

Calculate the equilibrium concentration of H4IO6-1 if the initial concentration of IO4-1 is 0.950 M and the Kc = 3.50. IO4-1(aq) + 2H2O(l) ↔H4IO6-1(aq) Group of answer choices 0.739 M 3.87 M 0.903 M 3.16 M 0.0704 M

Given these two reactions below: PbCl2(s) 2 Pb2*(aq) + 2CI(aq) Ksp = 1.17x10-5 Pb2+(aq) + 3 OH (aq) → Pb(OH)3 (aq) Kform 8x1013 determine the equilibrium constant for this reaction shown: PbCl2(s) + 3 OH (aq) Pb(OH)3 (aq) + 2CI'(aq) K = ? > O 4x10-11 O 2x10-17 O 7x10° O 9x108

.  What is the equilibrium constant for the neutralization of nitrous acid with ammonia? The Ka for nitrous acid is 4.5 × 10-4 and the Kb for ammonia is 1.8 × 10-5. 8.1 × 105 1.8 × 109 4.5 × 1010 8.1 × 1019 None of these are correct.

What are the Initial Concentrations of Fe3+ and SCN-? Fe3+ (aq) + SCN– (aq) à FeSCN2+ (aq) Flask # 0.2 M Fe(NO3)3 in 0.50M HNO3 0.50M HNO3 2.00 x 10–3 M KSCN in 0.50M HNO3 Initial [Fe3+] Initial [SCN-] Initial [FeSCN2+] Blank 5 mL 5 mL 0 mL       1 5 mL 4 mL 1 mL       2 5 mL 3 mL 2 mL       3 5 mL 2 mL 3 mL       4 5 mL 1 mL 4 mL       5 5 mL 0 mL 5 mL       Show a sample dilution calculation for flask 1. Hint: M1V1 = V2V2

How can I figure this out using solubility? I know I need to find a reagent that will form precipitate with Ag+ or Na+   You are the manager of a chemical stockroom, and find a bottle containing approximately one liter of a clear and colorless solution of unknown identity and concentration. Your only clue to its identity is that it was found between bottles of silver fluoride and sodium fluoride, so it is likely an aqueous solution of one of those two compounds. You will need to develop a procedure to determine the following: a) The identity of the unknown solution b) The concentration of the unknown solution

For cerium(III) hydroxide, Ce(OH)3, Ksp equals 2.0  10-20. Calculate its molarsolubility

Acetic acid partially dissociates according to the reaction below. HC₂H3O2 + H₂O(1) H3O+ + C₂H3O5 2 K 1.8 x 10-5 @ 25°C = Calculate the equilibrium concentrations of the components based on a 0.21 M acetic acid solution. What is the concentration of H3O+? [?] [H3O+] = [?] x 107] M

The following reaction in aqueous solution has Kc = 1 × 10-85 at a temperature of 25 °C. 7103(aq) + 9H₂0 + 7H*(aq) 1₂(aq) +5H5106(aq) What is the equilibrium law for this reaction? Ke = Ke Ke = Ke = [Hs 106]5 [103] [H+ ] [Hs 106]³[ 1₂ ] [103] [H+ ] [H5 106]³[ 12 ] [103] [H+ ][ H₂ O] [Hs 106]³ [103]

In a 1.0 x 10-6 M solution of Ba(OH)₂ (aq) at 25 °C, arrange the species by their relative molar amounts in solution. Ba(OH)2 H₂O Ba + H₂O* Greatest amount Least amount Answer Bank OH™

Equilibrium Lab- Post Lab Question Name Marlysa Rackmyre #13 A student prepares two flasks. Flask A contained 5.00 mL of 3M HCl(aq) (density 1.05 g/mL). Flask B contained 5.00 mL of 3M HCl(aq) and 5.00 mL of ethyl acetate (density 0.893 g/mL).Flask A and Flask B are titrated against a standard solution of NaOH(aq) after Flask B has attained equilibrium. The titration values and the molarity of the sodium hydroxide for your titrations are shown in the data table that follows. Use the data to calculate K, for the reaction shown below. EtAc + H₂O EtOH + HAC Titration reading Titration reading molarity of NaOH (ag) for flask A (mL) for flask B (ml) 2.737 5.28 12.42

1. Find the solubility of MgCO3 in water assuming a pH of 7.50. Ksp MgCO3=3.5 e-8 Ka1 H2CO3=4.45 e-7 Ka2=4.69 e-11 Step 1. Write all pertinent equilibrium reactions Step 2. Write the charge balance equation Step 3. Write the mass balance equation Step 4. Write the equilibrium constant for each chemical reaction Step 5. Count the equations and unknowns (# equations > # unknowns?) Step 6. Calculate the solubility of [Mg2+].

5. Equilibrium Lab- Post Lab Question Name Marlysa Rackmyre #13 A student prepares two flasks. Flask A contained 5.00 mL of 3M HCl(aq) (density 1.05 g/mL). Flask B contained 5.00 mL of 3M HCl(aq) and 5.00 mL of ethyl acetate (density 0.893 g/mL).Flask A and Flask B are titrated against a standard solution of NaOH(aq) after Flask B has attained equilibrium. The titration values and the molarity of the sodium hydroxide for your titrations are shown in the data table that follows. Use the data to calculate Ke for the reaction shown below. EtAc + H₂O EtOH + HAC Titration reading Titration reading. molarity of No OH (aq) for flask A (mL) for flask B (ml) 2.737 5.28 12.42

The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq)  which is a common ion then what would be the concentration of the Magnesium ion Mg2+(aq) in Molarity at equilibrium?   3.89 x 10-6   4.07 x 10-6   3.47 x 10-6   2.45 x 10-6   2.81 x 10-6   3.28 x 10-6   2.64 x 10-6   3.69 x 10-6   3.01 x 10-6   4.29 x 10-6

Predict the solubility product constant: Ag2CO3(s) 2Ag* (aq) + CO3-2(aq) Sample answer format: [Al+3][X-] *Put / or numbers outside the bracket if applicable

Determine the Ksp for magnesium hydroxide (Mg(OH)2) where the solubility of Mg(OH)2 is 1.4 × 10-4 M. A) 2.7 × 10-12B) 1.1 × 10-11C) 2.0 × 10-8D) 3.9 × 10-8E) 1.4 × 10-4

The solubility of CaSO4 (MM=132.6) is 0.191 g per 100 mL. Find the solubility product constant.     2.07 x 10-6     2.07 x 10-4     1.44 x 10-2     1.44 x 10-4

Will a precipitate form if a mixture contains (Ag+) = 1.2 x 10-4 M and (C2O4-2) = 4.7 x 10-3 M?    (Ksp = 3.5 x 10-11)                            Ag2C2O4 (s)  ⇔  Ag+ (aq)  +  C2O42- (aq)   What is the Q of the reaction?  Will it precipitate? (yes/no)    Format for scientific notation = 1.0 x10^-8

Will a precipitate form if a mixture contains (Ag+) = 1.2 x 10-4 M and (C2O4-2) = 4.7 x 10-3 M?    (Ksp = 3.5 x 10-11)                            Ag2C2O4 (s)  ⇔  Ag+ (aq)  +  C2O42- (aq)   What is the Q of the reaction?  Will it precipitate? (yes/no)

C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H* (aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.120 M, [H*] = 3.00 x 10-4 M, and [A- = 3.00 x 10-4 M. Calculate the Ka value for the acid HA. Ka : Incorrect

3. A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa).  [Ka= 1.8 x 10–5]   What is the new concentration of NaOH after dilution?   a 0.0273   b 0.0439   c 0.0185   d 0.0267   e 0.0385

Experiment 3, Part 2: Write the equilibrium equation for the saturated barium chromate solution. barium chromate equilibrium: BaCr₂O₂ (s) = Ba²+ (aq) + CrO² (aq)

The reaction A2+B2____2 AB has an equilibrium constant of kc=4

Benzoic acid, HC7H502, and its salts are used as food preservatives. Ka for benzoic acid is 6,3 X 1 0 -5 . A solution of sodium benzoate, NaC7H502, in water has a concentration of 0.015 mol.dm-3 .a) What is the equilibrium concentration of benzoic acid in the sodium benzoate solution?b) What is the pH of this solution?

A solution of 89.1 ml of 0.00185 M A₁B3 is mixed with a solution of 49.44 ml of 0.00800 M C₁D3. Find the value of pQ (the minus log of Q) for the formation of C₁B3. 8.1 9.89 4.99 5.47 11.32 8.35

2. Calculate the molar solubility of lead(II) phosphate in a pH 10 solution. Pb3(PO4)2(s) 3 Pb²+ (aq) + 2 PO4³- (aq) Pb²+ (aq) + 3 OH(aq) Pb(OH)3(aq) Ksp = 1.0 x 10-54 Kf = 8.0 x 1013 Pb3(PO4)2(s) + 9 OH(aq) 3 Pb(OH)3 (aq) + 2 PO4³- (aq)