Equilibrium Questions and Answers

Identify Sr(OH)2 (aq) as an acid or a base. acid base Part D Write a chemical equation showing how this is a base according to the Arrhenius definition. Express your answer as a balanced chemical equation. Identify all of the phases in your answ A chemical reaction does not occur for this question.

Consider two solutions, the first being 60.0 mL of 1.00 M CuSO, and the second 60.0 mL of 2.00 M KOH. When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from 23.5 to 29.7°C. a. Write the chemical equation showing the precipitation reaction being described. Clearly label the precipitate formed. b. Write the complete and net-ionic equations for the reaction that occurs when the two solutions are mixed.

A sealed container of methanol (CH3OH) contains both the liquid and gas in equilibrium: CH3OH(l)<->CH3OH(g) ΔH = +37.61 kJ/mol Indicate whether these changes would shift the equilibrium to the left or to the right.

Equilibrium describes the balance that results from a forward and reverse reaction proceeding at equal rates. Since reaction ratesdepend on concentration, temperature, and pressure, any changes in these conditions may alter the forward and reverse rates unequally and disrupt the equilibrium. Le Chatelier's principle states that after a change in conditions displaces a reaction from equilibrium the reaction proceeds to a new equilibrium in the direction that offsets the change. the reaction will undergo a temperature change in order to offset the disturbance. the disturbance will always cause the forward reaction to be slower than the reverse reaction. the change in conditions must be reversed in order to regain equilibrium.

A 5 mL sample of vinegar (HC₂H3O2(aq)) requires a 37.28 mL of 0.127 M NaOH to reach the equivalent point. What is the molar concentration of HC₂H3O2? The equation for the reaction is HC₂H3O2 + + NaOH -> NaC₂H3O2 + H₂O (Answer to 3 decimal places)

For the reaction A (g) → 3 B (g), Kp = 73900 at 298 K. When AG - -14.2 kJ/mol, what is the partial pressure of A when the partial pressure of B is 2.00 atm for this reaction at 298 K.

A 52.0-mL volume of 0.35 M CH3COOH (K₁ = 1.8 x 10-5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 23.0 mL of NaOH. Express your answer numerically.

A beaker with 185 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.10 mL of a 0.480 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( - ) sign if the pH has decreased.

An excess amount of Mg(OH)₂ is mixed with water to form a saturated solution. The resulting solution has a pH of 9.10. Calculate the solubility, s, of Mg(OH)₂ (s) in grams per liter in the equilibrium solution. The Ksp of Mg(OH)₂ is 5.61 x 10-¹2. S = 3.9 Incorrect g/L

When a chemical reaction is at equilibrium, the forward and reverse reactions occur at the same rate. The concentrations of the different compounds in the reactions will remain constant. The relationship between the concentrations of the reactants and products is expressed as the equilibrium constant, Ke. Determine the Ke expression for the reaction above by identifying what belongs in the numerator and what belongs in the denominator: =1/4 Drag each item to the appropriate bin. ► View Available Hint(s) Numerator [COC1,]2 [0₂]² [CCL]2 | |[C12]2 | numerator K= denominator Denominator [Cl₂] [CCL] [COC1] Not used Reset Help [0₂]

Classify each of these solids as ionic, molecular, metallic, or covalent (also known as covalent-network solids or macromolecular solids). Na₂S Ionic C(diamond) Na Molecular CC14 Answer Bank Metallic Covalent

5. A 500.0 ml solution of a buffered solution has a pH = 7.4. a) What is the [H3O+]? b) If a few drops of dilute HCl were added what would happen to the pH? c) If a few drops of dilute NaOH were added what would happen to the pH?

An excess amount of Mg(OH), is mixed with water to form a saturated solution. The resulting solution has a pH of 9.10. Calculate the solubility, s, of Mg(OH)₂ (s) in grams per liter in the equilibrium solution. The Ksp of Mg(OH)₂ is 5.61 x 10-12.

15. Provide the reactions that describe when H30* (acid) and OH (base) is added to the buffer solution. Normal = BIU Reaction of buffer with H₂O*(acid) Reaction of buffer with OH (base) X₂ X²→→→→→ III = fx &

The reaction between nitrogen and hydrogen to produce ammonia is described by the following equilibrium reaction. 3H₂ + N₂2 NH3 What substances are present in the reaction mixture when equilibrium has been obtained? ON₂ ] H₂ NH NH₂

At 850 K, the equilibrium constant for the reaction 2 SO₂(g) + O₂(g) = 2 SO, (g) is K. = 15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium.

In a saturated solution of an ionic compound in water, there is an equilibrium between the solid compound and the dissolved ions. The equilibrium expression for this type of reaction is called the solubility product constant, Ksp, which can be calculated from the concentrations, in moles per liter, of each ion in solution. For example, the solubility reaction and solubility product of barium carbonate, BaCO3, are BaCO3(s) = Ba²+ (aq) + CO3²- (aq) Ksp = [Ba2+][CO3²-] Similarly, the solubility reaction and solubility product of calcium sulfate, CaSO4, are CaSO4(s) Ca²+ (aq) + SO4²- (aq) Ksp = [Ca²+][SO4²-] = Part A The solubility of barium carbonate, BaCO3, is 0.0100 g/L. Its molar mass is 197.3 g/mol. What is the Ksp of barium carbonate? Express your answer numerically. ► View Available Hint(s) Ksp = Submit Part B VAE μА The solubility product constant of calcium sulfate, CaSO4, is 7.10 x 10-5. Its molar mass is 136.1 g/mol. How many grams of calcium sulfate can dissolve in 40.5 L of pure water? Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) Value Units Review I Constants I Periodic Table ? ?

The synthesis of methanol from carbon monoxide and hydrogen gas is described by the following chemical equation: CO(g) + 2H2(g): CH3OH(g) The equilibrium constant for this reaction at 25 °C is Kc = 2.3 x 104. In this tutorial, you will use the equilibrium-constant expression to find the 1 concentration of methanol at equilibrium, given the concentration of the reactants. ▼ Correct The equilibrium constant is expressed as Kc = [CH3OH] [CO][Hz]? Part B Review | Constants | Periodic Table The equilibrium-constant expression is a mathematical equation that can be rearranged to solve for any of the variables in it. Rearrange the equilibrium-constant expression to solve for [CH3OH]. ► View Available Hint(s)

The equilibrium constant, Kc, for the following reaction is 4.1x10-³. N₂O4 (9) 2NO2 (g) If the equilibrium mixture contains 0.045 M NO2, what is the molar concentration of N₂O4? Express your answer to two significant figures and include the appropriate units. μA ? [N₂04] = 4.94 moler The unit you entered is not recognized. Review a list of acceptable units. No credit lost. Try again. Bewer

Choose the equilibrium expression for each of the following reactions: Part C CH4 (9) + Cl₂(g) O Ko OK. = Ke Submail CH3CI(g) + HCl(g) = [C1₂][CH4] [HCI][CH, CI] [CHC1s][Cl₂] [CH][CH, CI] [HCI||CH,Cl| [C1₂][CH] Request Answer

Consider the following chemical reaction: Heat + 2 NOCI (g) 2 NO(g) + Cl2(g) Which of the conditions listed below will result in the equilibrium shifting toward the reactant side, according to Le Châtelier's principle? View Available Hint(s) increasing the concentration of NOCI (g) O increasing the concentration of C12(g) O heating the reaction O adding a catalyst

Ammonia, NH3, is used in numerous industrial processes, including the production of pharmaceuticals such as sulfonamide and antimalarials and vitamins such as the B vitamins. The equilibrium equation for the synthesis of ammonia (sometimes known as the Haber process) is N₂(g) + 3H₂(g) = 2NH3(g) Part A The Haber process is typically carried out at a temperature of approximately 500 °C. What would happen to the rate of the forward reaction if the temperature' were lowered to 100 °C? ► View Available Hint(s) The reaction rate would increase O decrease O not change

An equilibrium reaction has a Ke of 1.4 x 109. Which of the following accurately describes the chemical equilibrium for this reaction? ► View Available Hint(s) O The concentrations of the products are approximately the same as the concentrations of the reactants. O The concentrations of the reactants are less than the concentrations of the products. The equilibrium is said to favor the reactants. O The concentrations of the products are less than the concentrations of the reactants. The equilibrium is said to favor the reactants. O The concentrations of the products are greater than the concentrations of the reactants. The equilibrium is said to favor the products.

(7 pts.) Which of the following solutions will be the best buffer at a pH of 3.47? Please explain fully. (Please see the equation sheet for useful information). A) 0.10 M CH3NH2 and 0.10 M CH3NH3C1 B) 2.5 M CH3NH₂ and 2.5 M CH3NH3Cl C) 2.0 M HF and 2.0 M NaF D) 3.0 M CH3NH2 and 3.0 M HF

Ephedrine and its salt are used for a variety of disorders. Calculate the ratio of the acid form of the drug (ephedrine HCI) to the base form (ephedrine) in the stomach at pH 6.00. The pKa of Ephedrine is 9.6. (4 pts)

Calculate the pH of a solution prepared by dissolving 1.45 g of sodium acetate, CH3COONa, in 57.0 mL of 0.20 Macetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. K₂ of CH3COOH is 1.75 x 10-5.

A chemist fills a reaction vessel with 9.81 atm methanol (CH3OH) gas, 2.78 atm oxygen (O₂) gas, 9.08 atm carbon dioxide (CO₂) gas, and 5.38 atm water (H₂O) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 2CH₂OH(g) +30₂ (g) 2 CO₂(g) + 4H₂O(g) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule.

A chemist dissolves 472. mg of pure barlum hydroxide in enough water to make up 190. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places.

Task 1: Research (you should've done this in your checkpoint) If you are going to use red cabbage to make your own pH indicator, you first need to understand how a pH indicator works. Do some research into pH and how litmus paper can be used to measure it. Then research red cabbage and its relation to measuring pH. You'll need to document your sources as well. These are the sources that will eventually end up in your "References" part of the lab report. I've created a checkpoint in Summit to help guide you through this task.

A chemist dissolves 490. mg of pure barium hydroxide in enough water to make up 160. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places.

The preparation of an aqueous solution is described in the table below. For this solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH3 is a weak base. 0.4 mol of HNO3 is added to 1.0 L of a 0.4M NH3 solution.

Pay attention to the reaction letter as they are referenced throughout this section. Write equilibrium expressions for each following reaction a. NaOH(aq) + HCl(aq) -> H₂O(l) + NaCl(aq) b. K₂SO4 (aq) + Ca(NO3)2(aq) -> 2 KNO3 (aq) + CaSO4(s) c. 4NO(g) + 3O2(g) -> 2N2O5 (g) d. C3H8(l) + 5O₂(g) -> 3CO2(g) + 4H2O(l) e. 2 H₂O(l) -> 2H₂(g) + O₂(g)

Which is an example of a heterogeneous equilibrium system? Fe³+ (aq) + SCN- (aq) FeSCN²+ (aq) NO₂(g) + NO(g) = N₂O3(g) Cu²+ (aq) + 2OH(aq) = Cu(OH)2(s) 2H₂(g) + O₂(g) = 2H₂O(g)

Suppose that 8.00 mol of both O2 and N2O gases are introduced into a 4.00 L closed flask. When the system comes to equilibrium, 3.00 mol of nitrogen monoxide (NO) gas has formed. The reaction is shown below. Determine the equilibrium concentrations of all entities in the flask, NO, NO2 and 02. (6 marks) *SHOW YOUR WORK! 2N₂O(g) + O₂(g) = 4NO(g) DONE Not done

A chemistry student weighs out 0.168 g of acrylic acid (HCH₂CHCO₂) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1600M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits.

A certain ionic compound X has a solubility in water of 0.648 g/mL at 20. °C. Calculate the greatest mass of X that could be dissolved in 450. mL of water at this temperature. You may assume the volume of the solution doesn't change as the X is dissolved. Be sure your answer has the correct unit symbol and 3 significant digits.

In the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HCIO2(aq) + H2O(l) = H2O+ (aq) + ClO2- (aq) H2CO3(aq) + H2O(l) = H3O+ (aq) + HCO3-(aq) H2O(l) +CH3NH3+(aq) = CH3NH2 (aq) +H3O+(aq) CH3COOH(aq) + H2O(l) = CH3COO- (aq) + H3O+ (aq)

A certain organic compound O has a solubility in acetone of 0.799 at 5. °C. Calculate the mass of O required to prepare 650. mL of a saturated solution of O in acetone at this temperature. Be sure your answer has the correct unit symbol and 3 significant digits.

Which of the following is a nonelectrolyte? KI C6H12O6 (glucose) HF KOH

Consider the titration of 50.0 mL of 2.0 M HNO2 (K = 4.0x104, a weak acid) with 1.0 M KOH (a strong base). What is the pH at the equivalence point?

It is found that up to 0.0110 g of SrF2 dissolves in 100 mL of aqueous solution at a certain temperature. Determine the value of Ksp for SrF2.

Write a net ionic equation for the reaction that occurs when aqueous solutions of potassium hydroxide and hydroiodic acid are combined.

Calculate the number of milliliters of 0.697 M Ba(OH)₂ required to precipitate all of the Cr³+ ions in 197 mL of 0.414 M Cr₂(SO4)3 solution as Cr(OH)3. The equation for the reaction is: Cr₂(SO4)3(aq)+ 3Ba(OH)₂(aq) →→2Cr(OH)3(s) + 3BaSO4(aq) mL Ba(OH)₂

The precipitate of M₂S3 is obtained on mixing equal volumes of solution S₁ having [M³+] = 4 x 10-4 Mand S₂ having [S²] = 2 × 10-³ M. Calculate its solubility products. - A B C 4 x 10-17 108 × 10-17 54 x 10-17 D 8 x 10-17

Calculate the solubility at 25 °C of BaCrO4 in pure water and in a 0.0030 M BaCl₂ solution. You'll find Kp data in the ALEKS Data tab. Round both of your answers to 2 significant digits.

When an instant hot pack is activated, aqueous sodium acetate crystallizes to form a solid and heat is released. What are the signs of AHsys, ASsys, AGsys, Suniv? AH sys AS sys positive AG sys negative ASuniv impossible to determine As temperature increases, the reaction becomes spontaneous.

Calculate the solubility at 25 °C of Zn(OH)₂ in pure water and in a 0.0030 M ZnSO4 solution. You'll find K, data in the ALEKS Data tab. sp Round both of your answers to 2 significant digits.

Ozone, O, is an important absorber of UV radiation in our atmosphere. Upon absorption of UV radiation, O, dissociates into molecular oxygen, O₂, and a free oxygen atom. The free oxygen atom can then join with another O, molecule to create more ozone, which can in turn absorb more UV radiation. Alternatively, the free oxygen atom could join with O, to create more 0₂. 2 O3(g) →3 O2(g) The reaction would have a Why? -- -- AS.

A solution is prepared at 25 °C that is initially 0.41 Min trimethylamine ((CH₂), N). a weak base with K-7.4 x 10, and 0.35 M in trimethylammonium chloride ((CH₂), NHCI). Calculate the pH of the solution. Round your answer to 2 decimal places. PH-0

An analytical chemist is titrating 91.0 mL of a 0.4700 M solution of cyanic acid (HCNO) with a 0.7300 M solution of NaOH. The pK, of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 62.0 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. PH-0