Equilibrium Questions and Answers

Given a 0 01 M solution of the following three weak acids Acetic acid CH3COOH which has Ka 1 8x10 5 Nitrous acid HNO Ka 4 6x104 and Formic acid HCOOH Ka 1 8x10 4 Which solution has the lowest pH value Acetic acid All have the same pH value Formic acid Nitrous acid

A 0 010 M solution of cyanic acid has a pH of 2 76 Calculate the ionization constant Ka of the acid

Which of the following can behave as Bronsted Lowry bases in aqueous solution O H SO3 Br NH4 H SO4 O None of the Above

What is H O for a buffer solution that is 0 200 M in acid and 0 500 M in the corresponding salt if the weak acid s K 6 10 x 10 7 Enter your answer in scientific notation Be sure to answer all parts x 10 select M

Professor Bruns the same reaction given in problem 4 but starts from different initial concentrations of the reactants and products He places 4 0 mol of NH3 1 0 mol of N2 and 2 0 mol of H2 and in a sealed 1 0 L container at T 740 K What is the initial value of the reaction quotient in Professor Schwartz experiment A Qe 0 10 B Qc 0 50 O C Qe 1 0 D Qe 2 0 E Qe 10 0

Enter your answer in the provided box Use the Henderson Hasselbalch equation to calculate the pH of a buffer solution in which both the acetic acid and the sodium acetate concentrations are 1 5 x 10 M The equilibrium constant K acetic acid is 1 8 105 pH

The reaction 2A B g g has a value of Kp 8 43 If the reaction is initiated with 3 0 atm of gas A and 46 atm of gas B which direction will the reaction proceed to reach equilibrium Select one O a to the left creating more reactant b the pressure of all gasses will increase O c to the right creating more product O d the pressure of all gasses will decrease O e the system is already at equilibrium

For the equilibrium situation involving acetic acid CH3COOH aq H O CH COO aq H O aq explain the equilibrium shift that occurs when more acetic acid is added to the solution Select all apply The equilibrium will shift to the left The equilibrium will shift to the right The amount of H30 decreases The amount of CH3COO decreases The amount of CH3COO increases The amount of H O increases

Calculate the pH of a buffer system containing 1 0 M CH3COOH and 1 2 M CH3C K of acetic acid CH3COOH is 1 8 x 10 5 Enter your answer in the provided be Your Answer

What volume of 0 2000 M KOH is required to titrate 33 00 mL of 0 3000 M HNO Enter your answer in the provided box mL KOH

Be sure to answer all parts attempts Calculate the pH of a solution that is 4 2 x 10 Min HNO3

Write an equation for the reaction of HSO with water Click in the answer box to activate the palett aq aq ag

23 nts 1 attempt left Check my work Which of the following are capable of forming a buffer solution HBr and MgCl H CO3 and NaHCO3

attempts Check my work Calculate the pH of a 0 0023 M solution of KOH Enter your answer in the provided box

What is the H O concentration of a solution with a pH of 5 1 Enter your answer in scientific nota Be sure to answer all parts x 10 select M

Click in the answer box to activate the palette Write the formula of the conjugate acid of Br

x 10 Be sure to answer all parts Enter your answer in scientific notation Calculate the H3O of a solution of HNO3 with pH 6 00 H O select pis M Check my work

Enter your answer in the provided box Calculate the pH of a solution with a H O concentration of 1 3 10 6 M

SIMULATION Hydrolysis ONa O NH4 O C5H5NH SOCI OF O CN O NO O CIO Concentration 0 01 M NaCl pH 7 00 Now explore the effect of changing the anion Make a 0 10 M solution of NaF What is the pH of that solution 123 56 7 8 7 00 9 11 12 13 14

Problem Statement Estimate how many Rolaids tablets are required to neutralize all the acid in one glass 250 mL of a regular cola drink Assume that cola drink pH 3 0 one Rolaids tablet contains 334 mg of NaAl OH 2CO3 To make this estimate assume that the pH indicates the total concentration of acid in the cola Then figure out how many moles of H aq are present in the acidic cola drink and how many moles of H aq each tablet can consume Let s start with the first part First Step in Solution Calculate the H aq in a pH 3 0 solution X mol L

to describe the proton transfer that occurs when each of these acids is added Use the lowest possible coefficients Be sure to specify states such as aq or s If a box is not needed leave it blank a b C HCO3 HCI Submit CH3COOH water

Chemistry Write the balanced chemical equation for the equilibrium of lactate ion in water

b Highly electronegative atoms lead to stronger acids Now consider the following two bases BrNH and NH3 Which of these will be the stronger base O O BrNH2 NH

Predict whether this acid base reaction is product favored or reactant favored NH4 aq Br aq O O product favored reactant favored there are not enough data

Choose the correct symbol for the equilibrium constant of the autoionization of water 2H O 1 OH aq H30 aq K H3O OH O kp O kw O kw kp

parts to get a Designate the acid and the base on the left side of this equation Hl aq H O l H30 aq aq Select all that apply acid Hl aq acid H O l base Hl aq

Calculate the Keq from the given concentrations MgCl and K CO3 were dissolved and the reaction happened because a solid was formed 2 KC Mgale c a 1 00 M 0 300 M 0 1 40 M 0 700 M start equil K CO 1 00 M 0 300 M 0 700 M Keq First put in the chemicals then put in the numbers The concentration of KCI was squared due to its coefficient 1 2 1 MgCO 0 N A Keq a H301 b OH C K CO3 1 C H30 J H S k HS 1 s 0 300 t 0 333 r 0 250 y 0 7000 z 1 60 x 10 5 d MgCO3 e MgCl f KCI 8 H SO3 1 5 m HX n x u 1 40 v 1 75 x 10 5 o 0 750 W 1 11 x 10 8 aa 1 143 x 105 bb 0 500 CC 1 104 x 10 5 h HC H 0 p 2 q 1 x 5 5 x 10 dd 0700

a Solution A has a pH of 3 and solution B a pH of 6 Which has the greater hydronium ion concentration O solution A O solution B O the concentrations are equal

TUTOR Strong Bases Calculate pH What is the pH of a 1 7x10 2 M solution of KOH at 25 C

Choose the correct definition for a supersaturated solution in terms of Q and Ke O If the concentration of the solution phase solute is smaller than the equilibrium concentration then Q K and the solution is supersaturated O If the concentration of the solution phase solute is the same as the equilibrium concentration then Q K and the solution is supersaturated O If the concentration of the solution phase solute is greater than the equilibrium concentration then Q Ko and the solution is supersaturated O If the concentration of the solution phase solute is greater than the equilibrium concentration then Q K and the solution is supersaturated

Give the expression for Keq for the forward reaction All are gases in a closed container C H6 2Cl C H4Cl2 2HCI The concentrations for both Cl and HCI are squared due to their coefficients 1 Keq a H30 b OH1 i C H30 J H S s 5 5 X 105 r 0 5000 x 5 5 x 10 2 dd 0 7100 00 C C H6 d C H4Cl2 k HS1 1 S t 3 5 x 104 z 1 60 x 10 5 ff 901 y 0 7000 ee 1 26 x 105 e Cl m HX u 8 00 x 105 a 1 143 x 105 ga 7 02 1 f HCI n x g H SO3 0 1 v 1 75 x 10 6 h HC H302 q 3 p 2 w 1 11 x 108 cc 1 104 x 10 5 bb 0 4900

Use Le Chatelier s Principle to answer the following 1 What happens to the Is if the pH is lowered by adding H the added H is the same as adding H30 because H 2 H 0 52 H S 21 0 2 What happens to the Is the added OH reacts with H O and H S 2H O 3 H D H O 6 Hy if the pH is increased by adding NaOH 2 H30 52 the H O H 0

Calculate the pH of the buffered solution if at equilibrium H SO3 3 50 X 10 M HSO 5 5 X 102 M and K 1 75 x 105 everything is based upon the acid dissolving in water H SO3 H OHSO3 H 0 I solve for H 0 then put in the numbers K H 0 H 0 X

A buffer was made with HC H O and its conjugate base What is the pH of the buffer if at equilibrium there was HC H30 0 5000 M and C H O 0 7000 M and the K 1 60 x 105 everything is based upon the acid dissolving in water HGHEOz H GHO2 HO solve for H O then put in the numbers K H 0 H 0 pH log X

Calculate the pH of the above buffer after 10 00 mL of 1 000 M NaOH 0 01000 mol OH was added to 1 000 L of the buffer solution The new concentrations are HC H30 0 4900 M and C H30 0 7100 M The K 1 60 x 105 everything is based upon the acid dissolving in water HC H302 H O C H30 H30 1 Ka solve for H3O then put in the numbers Ka H301 H30 pH log 1

A buffer was created using ascorbic acid and sodium ascorbate What is the pH of the buffered solution if at equilibrium H C6H606 5 5 X 10 M HC6H606 3 5 X 104 M and K 8 00 x 105 everything is based upon the acid dissolving in water H C6H6O6 H O HC6H606 H30 1 solve for H O1 then put in the numbers Ka I H O 4

Which of the following would make a good buffer pair a weak acid and a weak base HCI and NaCl a yes b no H3PO4 and NaH PO4 HNO3 and NaNO3 H SO4 and NaHSO4 NaHSO3 and Na SO3 c what the heck

0 150 M hydrofluoric acid HF a weak acid K 7 2 x 10 4 M

For the reaction S F6 g 25F2 g F2 g the equilibrium concentrations are as follows 2F6 0 000430 M SF 2 08 M F 1 1 32 M The equilibrium constant is none of the above 1 19 x 10 4 8 43 x 103 O 1 33 104 7 53 x 10 5

A reaction that has Keq 2 0 x 108 will have high concentrations of products True False

The equilibrium expression for the reaction C s 2H g CH4 g is Kaq 1 True False CH 4 C H P

Write the overall molecular equation for the reaction of hydroiodic acid HI and potassium hydroxide Include physical states Enter the formula for water as H O molecular equation

Write the net ionic equation for the acid base reaction Include physical stat HI aq LiOH aq H O 1 Lil aq

Dissolving the compound PbCl2 into water can be represented as PbCl2 s Pb2 aq 2 C aq so the equilibrium expression is Ksp Pb2 1C 2 PbCl True False

The equilibrium expression for the reaction 2C s 2H O 1 CH g CO2 g is K CH4 CO True False 1

O a 3 3x10 11 O b 4 8x10 21 O c 3 0x10 4 O d 2 0x10 1 O e 7 3x10 10 A buffer solution is prepared with 0 580 M of hypochlorous acid HCIO and 0 711 M of sodium hypochlorite NaCIO For HCIO K 2 4 x 10 8 What is the pH of this solution Record you answer to 2 decimal places Answer holow This figure depicts

The reaction below is exothermic 2SO2 g O2 g 2SO3 g Le Chateliers Principle predicts that reaction container Select one O a adding a catalyst O b removing some O2 g O c adding some O2 g O d increasing the temperature O e removing some SO2 g will result in an increase in the number of moles of SO3 g in the

A 42 55 mL solution of weak acid is titrated with 0 471 M NaOH It requires 24 47 mL of the NaOH titrant to reach the equivalence point Based on the titration curve it is determined that Ka 7 6 x 10 8 for the weak acid Based on this information what was the pH after 30 93 mL of NaOH was added Write your answer to 2 decimal places ie 1 23 or 12 34 Answer At a certain temperature silver bromide AgBr has a value of Ksp 6 5 x 10 13 At this temperature what is the molar solubility of AgBr in the presence of 0 0044 M HBr Report your answer to two significant figures i e 1 2E 10 M

In an experiment 1 384 mol of CO g and 1 673 mol of H O g were placed into an empty 1 00 L reaction vessel At equilibrium there were 0 199 mol of CO g remaining Under these reaction conditions Kc is Record your answer to 3 significant figures Use scientific notation i e 1 23E 4 An evacuated i e empty vessel is charged with 0 847M of HI g The following reaction proceeds to reach equilibrium 2HI g H g 12 g The equilibrium constant for this reaction at this temperature is Kc 0 591 What is the concentration of hydrogen gas in this system at equilibrium Report your answer to 3 significant figures M

A gas mixture is prepared containing 0 538 moles of helium and 0 438 moles of argon This mixture is placed in a 1 87 L container at 33 1 C What is the total pressure under these conditions Please report the pressure in atmospheres to 3 significant figures