In the laboratory, a general chemistry student measured the pH of a 0.386 M aqueous solution of ethylamine, C,H&NH, to be 12.094. Use the information she obtained to determine the K, for this base. K,(experiment)-
Q: Calculate the pH at any point for an acid-base titration curve?
A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…
Q: In the laboratory, a general chemistry student measured the pH of a 0.546 M aqueous solution of…
A: Since you have posted multiple questions which are not sub-parts, we are entitled to answer the…
Q: In the laboratory, a general chemistry student measured the pH of a 0.528 M aqueous solution of…
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Q: A 0.085 M solution of a monoprotic acid has a percent ionization of 0.59%. Determine the acid…
A: Let the monoprotic acid be HA. HA dissociates as: Where c is the concentration of the acid, HA…
Q: In the laboratory, a general chemistry student measured the pH of a 0.546 M aqueous solution of…
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Q: Determine the % ionization of a solution of boric acid that is 60mM.
A: Given that, Concentration of boric acid = 60 mM Ka constant of boric acid = 5.9×10-10 In general,…
Q: In the laboratory, a general chemistry student measured the pH of a 0.453 M aqueous solution of…
A: pH = 12.155 Therefore, pOH = 14 – 12.155 pOH = 1.845 So,as we know that ; [OH¯] = 10¯pOH =…
Q: A solution is prepared that is initially 0.22M in methylamine (CH, NH,), a weak base, and 0.31 M in…
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Q: What is the relationship between the acid ionization constant for a weak acid (K.) and the base…
A: A species which donates protons is acid and a species which gains proton is a base. The values of pH…
Q: An aqueous solution of 0.1 M hydrochloric acid with a volume of 200 milliliters is mixed with 100 mL…
A: Moles of HCl taken = molarity of HCl X volume of HCl solution taken in L Since molarity of HCl = 0.1…
Q: The compound methylamine, CH,NH,, is a weak base when dissolved in water. Write the K, expression…
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Q: pH of a given buffer solution does not depend, in general, on concentration of buffer components.…
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Q: Why is there a need for buffers? Please explain in depth and detail
A: A buffer solution is a solution that can withstand changes in pH on addition of acidic or basic…
Q: A solution is prepared that is initially 0.36M in trimethylamine ((CH3),N), a weak base, and 0.19M…
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Q: In the laboratory, a general chemistry student measured the pH of a 0.598 M aqueous solution of…
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Q: Four unlabeled beakers in laboratory are filled with solutions of the following compounds: Na,S,…
A: In the given problem we are provide with four unlabeled beakers consisting of any of the following…
Q: A small amount of sodium hydroxide is added to water. When the chemical reaction reaches…
A: pH + pOH = 14 So, pOH = 14 - pH
Q: In the laboratory, a general chemistry student measured the pH of a 0.453 M aqueous solution of…
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Q: measımeasurement of PH of a solution can be use. or .....
A: The correct answer about pH is given below
Q: a the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of…
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Q: At the equivalence point of a weak base against HCl, the solution contains only that of the base,…
A: ITS FALSE AS TITRATION OF WEAK BASE AND STRONG ACID SUCH AS HCL GIVES OVERALL ALL ACIDIC SOLUTION…
Q: Calculate the K, for an unknown base, B, given that a 0.400 M solution of the salt HBCI has a…
A: Percent ionization, α % = 0.03 Concentration, C = 0.4 M
Q: In the laboratory, a general chemistry student measured the pH of a 0.455 M aqueous solution of…
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Q: Would a 1 M solution of just acetic acid resist increases to pH, decreases to pH, neither, or both?…
A: 1M acetic acid is acidic, because Ka value of acetic acid is greater than kb value of its conjugate…
Q: In the laboratory, a general chemistry student measured the pH of a 0.545 M aqueous solution of…
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Q: Which things should be considered while deciding weak acid/conjugate base pair to make a buffer…
A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…
Q: Briefly explain the approximate value of the pH at equivalence point.
A: The equivalence point is said to be achieved when moles of acid and base titrating are equal in…
Q: When is it safe to assume that the change from initial concentration (+/- x) is small enough to be…
A: When % of dissociation of weak acid or base is very small then the change from initial concentration…
Q: The pH of the solution obtained when 1.00 g of NaOH solid is added to 500 mL of 0.100 M HC2H3O2…
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Q: A solution is prepared that is initially 0.17 M in trimethylamine ((CH,),N), a weak base, and 0.20 M…
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Q: A few small drops of water are left in a burette that is used to titrate a base into an acid…
A: If the acid concentration is low then it will not affect too much since small amount of water will…
Q: In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of…
A: The base (B) isoquinoline C9H7N in aqueous solution can be represented as,…
Q: Enough of a monoprotic acid is dissolved in water to produce a 1.55 M solution. The pH of the…
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Q: What should the pH be for a 0.1 M solution of a strong monoprotic base
A: Strong base are those base which dissociate 100% and gives OH- ion on dissolution. From the…
Q: If the total concentration of a buffer is known (and not the individual concentrations of the weak…
A: Buffer solution: It is the aqueous solution that consists of a weak acid and its conjugate base or a…
Q: A 1.0 M solution of hydrochloric acid is mixed with an equal volume of sodium hydroxide solution.…
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Q: What simplifying assumptions do we usually make in working problems involving equilibria of salts of…
A: Since this question contains multiple parts, the answer for first three questions are given below.…
Q: Discuss how buffers help prevent drastic swings in pH. Explain in details information.
A: Discuss how buffers help prevent drastic swings in pH. Explain in details information.
Q: In the laboratory a student measures the percent ionization of a 0.558 M solution of formic acid ,…
A: The dissociation of formic acid: Concentration of formic acid =0.558M. Percentage ionization of…
Q: In the laboratory, a general chemistry student measured the pH of a 0.446 M aqueous solution of…
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Q: a. Calculate for the concentrations of the five standard solutions
A: A question based on concentration terms that is to be accomplished.
Q: What is the value of K.
A: A + B = C + D (reaction at equilibrium) Kc = [product]/[reactant] Kc = [C].[D]/[A].[B] Where…
Q: In the laboratory, a general chemistry student measured the pH of a 0.528 M aqueous solution of…
A: Isoquinoline is a weak base pOH = 14 - pH pOH = -log [OH-] For a weak base: [OH-] = (Kb x C)1/2…
Q: If 50mL of 0.10M NaOH is added to 50mL of 0.10M monoprotic weak acid, the resulting pH of the…
A: This can be calculated using Henderson -Hasselbalch equation
Q: A solution is prepared that is initially 0.069M in ethylamine (C,H,NH,), a weak base, and 0.15M in…
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Q: Addition of the indicator methyl orange to an unknownsolution leads to a yellow color. The addition…
A: a) Given: Addition of phenolphthalein: No color change Addition of bromthymol blue: Yellow color…
Q: In the laboratory, a general chemistry student measured the pH of a 0.469 M aqueous solution of…
A: Therefore ka for acetic acid is 1.9186* 10-5
Q: Enough of a monoprotic acid is dissolved in water to produce a 1.07 M solution. The pH of the…
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- Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionEstimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
- Use the data in Table 15.1 to select a conjugate acid-base pair you could use to make buffer solutions having each of these hydrogen ion concentrations. 3.2 × 10−4 M 5.0 × 10−5 M 7.0 × 10−8 M 6.0 × 10−11 MIonization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.The reaction just described is reversible. Deprotonation of the conjugate acid of an organic base by water provides another example of simultaneous making and breaking of sigma bonds. Thus, in the deprotonation of anilinium ion by water, the base is water, which has unshared electrons on the ________ atom. The acid is ________ ion. A pair of ________ electrons on the oxygen atom of water is pushed toward the ________ atom. Simultaneously, the pair of ________ electrons between the hydrogen and ________ atom of the anilinium ion is pushed toward the ________ atom. Thus, the oxygen- ________ sigma bond is made and a hydrogen- ________ sigma bond is broken. The nitrogen atom, which possessed a positive charge, is now ________, and the oxygen atom, which was neutral, now possesses a formal ________ charge.
- A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The final volume of the solution is 375 mL and the pH of this solution is 4.45. a What is the molar concentration of the sodium acetate? b How many milliliters of sodium hydroxide were added to the original solution? c What was the original concentration of the acetic acid?For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?