The Ką of acid HA is 3.5 x 10 and the Kp of base B is 7.2 x 104. When 0.50-mol HA and 0.50-mol B are mixed in 1 L solution, the pH of the final solution should be
Q: When 0.412 g of a weak base with Kb = 3.10 ×10-5 the base is dissolved in 1.00 L of solution, it has…
A: Assuming the molar mass is M Hence moles of base = mass / molar mass = 0.412 / M And concentration…
Q: A buffer solution is 0.316 M in CH;COOH and 0.275 M in CH3COON . If K, for CH;COOH is 1.8×10³ , what…
A: Concentration of CH3COOH=0.316M Concentration of CH3COONa=0.275M Ka of CH3COOH=1.8×10^-5 pH=?
Q: A solution is prepared at 25 °C that is initially 0.17M in acetic acid (HCH,Co,), a weak acid with…
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Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…
A: In order to find Ksp of the salt we first write down the given data: pH= 10.34. The given salt is…
Q: A solution is prepared at 25 °C that is initially 0.21M in propanoic acid (HC, H,CO,), a weak acid…
A: Buffer solution is mixture of weak acid and its salt. Here acid used is Propanoic acid and salt is…
Q: A solution is prepared by dissolving 0.89 mol of a weak base in 1.00 L of water. The resulting pH at…
A: Dissociation of a weak base and pOH calculation
Q: Two acids are mixed in solution: 0.20 M of HBr and 1.50 M of HBRO (Ka = 2.3 x 10-9). What is the…
A: HBr is a strong acid while HBrO is weak acid and therefore, the resulting pH will be due to HBr,…
Q: If a buffer solution is 0.170 M in a weak base (Kb = 4.2 × 10-5) and 0.490 M in its conjugate acid,…
A: Buffer solution: It is an aqueous solution which contains a mixture of a weak base and its conjugate…
Q: If a buffer solution is 0.200 M in a weak base (Kp = 6.4 x 10-) and 0.480 M in its conjugate acid,…
A: Again. pH= 14 - pOH Using these two formula pH of the solution can be calculated.
Q: Question 3 I'm not sure how to solve this question.
A: We assume 1L of solution Adding 16g of HBr Moles of HBr added = 16/80.91 = 0.197 moles
Q: A 245.0 mL sample of 0.15 M Ba(OH)2 is added to 438. mL of 0.20 M HNO3. What is the pH of the…
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Q: Calculate the pH of a solution containing 0.1M NH,OH and 0.01M NH.CI, K = 1.76 x 10$. %3D
A: Given, [NH4OH] = 0.1 M [NH4Cl] = 0.01 M Kb = 1.76 × 10-5
Q: What would be the pH if 1.11 moles of hydrofluoric acid (HF) were added to 2 liters of pure water,…
A: Given : Number of moles = 1.11 pKa = 3.2 HF ⇔…
Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…
A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…
Q: The PH of 0.0296M HA ( Ka 8.4 *10-9) plus * . . 0.1026 M NaA is 4.3 2 O 8.6 7.5 O
A: The question is based on the concept of PH calculations. we have been given a weak acid and its…
Q: 2) What is pH of the following weak acids" a. 0.01 M NH4CI b. 0.01 M NH3 c. 0.01 M NHẠCI added to an…
A: PH = -log ( H+) For aqueous solution highest PH at 25°C = 14 but non-aqeous solution it can be…
Q: If a buffer solution is 0.170 M in a weak base (?b=3.7×10−5) and 0.540 M in its conjugate acid, what…
A: In question it is not mentioned whether the base is monoprotic or polyprotic. Hence assuming it to…
Q: Fill in the left side of this equilibrium constant equation for the reaction of carbonic acid…
A: in this question given ka ka= Acid dissociation constant, acid dissociation constant is used to…
Q: Calculate the pH of the solution that contains 0.145 M NH3 and 0.192 M NH4Cl. The Ka of NH4+ is…
A: The solution will be the buffer solution if the weak acid and its corresponding conjugate base are…
Q: 0.0500 M HF (Ka= 7.20 x 10–4) determine the equilibrium molar concentration of H3O+ and…
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Q: If the Kp of a weak base is 1.0 x 106, what is the pH of a 0.11 M solution of this base? pH =
A: Let us consider a base B, hydrolysis of the base is given below B + H2O ---> BH+ + OH- Now, at…
Q: 0.1 M NH4CI solution, using the given pH data, write expression for equilibrium constant (Ka or Kb):
A: Net ionic reaction for the hydrolysis reaction in NH4Cl is given below NH4+(aq) +…
Q: ulate the pH of a solution prepared by dissolving 1.90 g of sodium acetate, CH,COONA, in 85.0 ml of…
A: Given, Mass of Sodium Acetate = 1.90 g Ka of CH3COOH is 1.75×10-5.
Q: Consider 20.00 mL of a 0.40M hypothetical weak acid solution, HA. The K, = 3.3 X 106 for this weak…
A: Given: Volume of weak acid, HA = 20.00 mL Molarity of HA = 0.40 M Volume of NaOH = 20.00 mL Molarity…
Q: If the K of a monoprotic weak acid is 1.8 x 10-6, what is the pH of a 0.35 M solution of this acid?
A: Given: Ka of weak monoprotic acid (Assuming HA) = 1.8 × 10-6 And the concentration of HA = 0.35 M
Q: If a buffer solution is 0.230 M0.230 M in a weak base (?b=7.4×10−5)Kb=7.4×10−5) and 0.540 M0.540 M…
A: we have to calculate the pH of the given buffer solution
Q: Given lead (I1) hydraxide Pb (OH),what is the molar solubility? K" 1.2x10 iwhat is the pH of this…
A: Since you have posted multiple questions, we are entitled to answer the first only.
Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?
A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…
Q: The concentration of CH3COOH (pKa=4.75) in vinegar is about 1.0 M. With this what do you predict the…
A: pH is the negative logarithm of Hydrogen ion concentration. pH of a solution can be calculated as:…
Q: A 0.15M solution of a weak base has a pH of 9.08. What is Kp for this weak base?
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Q: If the K of a monoprotic weak acid is 1.4 x 10-6, what is the pH of a 0.14 M solution of this acid?…
A: Given : Ka of monoprotic acid (assuming HA) = 1.4 X 10-6 And Concentration of acid = 0.14 M Since…
Q: If the Kp of a weak base is 2.5 x 10-6, what is the pH of a 0.23 M solution of this base?
A: pH + pOH = 14 For a weak base solution: [OH-] = (Kb x C)1/2 Where, C = molar concentration of weak…
Q: 2. If you make a solution by mixing 25.mL of 0.50 M acetic acid (CH3COOH) and 25 mL of 0.30 M sodium…
A: Given, [CH3COOH] = 0.50 M Volume of CH3COOH = 25 mL [CH3COONa] = 0.30 M Volume of CH3COONa = 25…
Q: 20 ml of 0.2 M NaOH solution be treated with 40 ml of 0.2 M acetic acid solution to give 60 ml.…
A: An acidic buffer is defined as an aqueous solution that consists of a mixture of a weak acid and its…
Q: What is the pH of a sodium acetate (NaCH3CO2) solution prepared by adding 0.820 g of sodium acetate…
A: Given: Mass of sodium acetate = 0.820 g Volume of water = 100.0 mL Ka of acetic acid…
Q: What is the pH of a 0.681 M weak base solution? The Kp of the weak base is 0.000098.
A: Given:: Let HB is weak base then, [HB] =0.681 M Kb=0.000098
Q: What is the pH for a weak monoprotic acid if a 0.020 M solution of the acid has a Ka of 3.28 x 10-7…
A: The H3O+ concentration for the weak acid is determined given below:
Q: If 10 mL of 0.1 M hypothetical acid, HA, is added with 10 mL of 0.1 M of the salt of its conjugate…
A: Answer: The mixture of acid HA and its conjugate base XA will be a buffer solution.
Q: A 0.15 M aqueous solution of a weak acid (HA) has a pH of 4.55 at 25 C. What is the ∆G for the…
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Q: If the K of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH =
A:
Q: Calculate the pH of a 0.10-M solution of aluminum chloride, which dissolves completely to give the…
A: The hydration of aluminum chloride to furnish [Al(H2O)6]3+ ion is expressed as follows:…
Q: Determine the pH of a solution by adding 0.23 mole formic acid and 0.17 mole of sodium formate in…
A: Here formic acid is a weak acid and sodium formate is an salt of weak acid so they both combine to…
Q: What mass of sodium acetate, NACH3 CO2 , must be added to 1.00 L of 0.080 M acetic acid to give…
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Q: If the Kp of a weak base is 7.3 x 10-6, what is the pH of a 0.28 M solution of this base? pH =
A: The value of Kb for the given weak base is = 7.3x10-6 The concentration of the base solution is =…
Q: A 0.437 M solution of a weak base has a pH of 11.94. What is the base hydrolysis constant, Kp, for…
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Q: HCIO is a weak acid (K. = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…
A:
Q: If the Kp of a weak base is 1.8 x 10-6, what is the pH of a 0.24 M solution of this base? pH =
A: Below attached file showing the details answer. All the best.
Q: If the KbKb of a weak base is 1.6×10−6,1.6×10−6, what is the pH of a 0.18 M0.18 M solution of this…
A: Concentration of the solution is 0.18 M. Kb = 1.6 x 10-6 The Ka value is calculated by following…
Q: What is the molarity of a solution made by dissolving 3.4 g of Ba(OH)2 in enough water to make 450.…
A:
Answer: greater than 7
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- Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
- 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.)An aqueous solution of 0.057 M weak acid, HX, has a pH of 4.65. What is the pH of the solution if 0.018 mol of KX is dissolved in one liter of the weak acid?Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?
- Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/AThe simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
- Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?Define or illustrate the meaning of the following terms: a. amphoteric b. Kw reaction c. Kw equilibrium constant d. pH e. pOH f. pKw Give the conditions for a neutral aqueous solution at 25C, in terms of [H+], pH, and the relationship between [H+] and [OH]. Do the same for an acidic solution and for a basic solution. As a solution becomes more acidic, what happens to pH, pOH, [H+], and [OH]? As a solution becomes more basic, what happens to pH, pOH, [H+], and [OH]?A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?