After creating a graph of pH versus log([Hln]/[In-1), the following trendline is obtained. y = -1.0970x + 3.898 Calculate the pKa of bromophenol blue from this data to three decimal places. Your Answer: Answer
Q: given that pka for nitrite ion ( NO2-) is 10.85 , find the quotient in (HNO2/NO2-) a solution of…
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A: Acid Ionisation constant Ka = 5.44*10-6 Let us suppose Ionisation constant for conjugate base is…
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A: Given, [HC5H9O2]=0.24 M pH=2.73 Ka= ?
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A: First Concentration of OH- is dind out and then pOH. And we know that pH + pOH =14
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Q: Vhat is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.26 at 25°C? (Ka for…
A: Formic acid, HCOOH is a weak acid. That's why pH = 1/2pKa - 1/2logC or, logC = pKa-2*pH ....(1)…
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Q: At 25°C, what is the hydronium ion concentration ina. 0.200 M chloroacetic acid? b. 0.0200 M…
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A: Normal Values pH = 7.35-7.45 pCO2 = 35-45 mmHg [HCO3-] = 22-26 mEq/L
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Q: The base protonation constant Kg of 1-H-imidazole (C,H,N,) is 9.0 x 10. Calculate the pH of a 0.24 M…
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A: Given : We have to calculate the pH.
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A: c = 0.98 M pH = 2.43
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Q: The base protonation constant K, of lidocaine (C14H„NONH) is 1.15 × 10°. Calculate the pH of a 0.86…
A: Given, Kb of lidocaine, C14H21NONH = 1.15 × 10-8 Concentration of lidocaine = 0.86 M
Q: Wgat is the [OH-] of a bleach sample that registers 11.41 on a pH meter?
A: The registered pH of a bleach sample on a pH meter is 11.41 pH = 11.41
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Q: The base protonation constant K, of azetidine (C,H,NH) is 1.5 × 10 Calculate the pH of a 1.1 M…
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Q: Calculate the pH at 25°C of a 0.58M solution of pyridinium chloride C5H5NHCl . Note that pyridine…
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Q: f the Kb of a weak base is 8.7E-9, what is the Ka of its conjugate acid?
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Q: The base protonation constant K, of 1-H-imidazole (C,H,N,) is 9.0 x 10°. -8 Calculate the pH of a…
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Q: Calculate the pH of an aqueous solution that is 0.35 M NH3 and 0.15 M NH,NO3 given that the K, of…
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A: We have to predict the pH of solution.
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Q: A solution is prepared at 25 °c that is initially 0.43M in methylamine (CH,NH,), a weak base with…
A: Given: Concentration of CH3NH2 = 0.43 M Concentration of CH3NH3Br = 0.13 M And Kb of CH3NH2 = 4.4 ×…
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Q: For H2S, Ka1 = 9.6 10-8, and since Ka2 = 1.3 10-14, 0.04 M Na2S Calculate the pH of the solution by…
A: Given, Ka1 = 9.6×10-8 and Ka2 = 1.3×10-14
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A: Given: Concentration = 0.150 M Ka of propanoic acid = 1.3 × 10-5 since propanoic acid is weak acid.…
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A: Given pKb for NO2- = 10.85 For HNO2 pKa = pKw - pKb = 14 - 10.85 = 3.15 Ka = 7.1 x 10-4 Chemical…
Q: Calculate the percent dissociation of 4-chlorobutanoic acid (C3H CICO₂H) in a 4.9M aqueous solution…
A: We would write dissociation equation of 4-chlorobutanoic acid as use its Kb value .
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- Calculate the percentages of dissociated and undissociated forms present in the following solutions: (a) 0.0010 M glycolic acid (HOCH2CO2H; pKa = 3.83) at pH = 4.50 (b) 0.0020 M propanoic acid (pKa = 4.87) at pH = 5.30What hydrogen ion concentration (H+) (expressed in mol dm - 3 ), corresponds-to a pH of 2.60? Give your answer to two decimal places and in scientific notationCalculate at what pH about 80% of 2-naphthol (pKa = 9.5) will be found in the ionized form in aqueous solution. Write your answer in numerical form with one diciminal digit (e.g. 1.1) Answer:
- Q2-3:(a) Given that Kb for ammonia is 1.8 X 10 -5 and that for methylamine is 4.4 X 10 -4, which is the stronger base? (b) which is the stronger acid ,the ammonium ion or the methylammonium ion ? (c) calculate the Ka for NH,* and CH;NH;* + Q2-4: A particular sample of vinegar has a pH of 2.90, assuming that the vinegar contains only acetic acid (Ka acetic acid in vinegar . 1.8 X 10 -5), calculate the concentration of Q2-5: Calculate the molar concentration of OH-ions in an 0.85M solution of hypobromite ion , BrO- (Kp 4.0X10-6) .what the pH value of this solution?ezto.mheducation.com Assignments: FA21:.. M Connect Sign In | M... M1-Hw Ch 9: 1-7- C... M9-Hw Ch 9: 9-11 -... 11 Saved The products are favored in the acid-base reaction: HI(aq) + NH3(aq) 2 NH4 (aq) +1(aq). True or False True FalseUse the References to access important values if needed for this question. The K, of a solution can be determined from the pKp using the equation: 10-pK, Kb Where: K = base dissociation constant a Use the rules for logarithms and exponents to solve for pKb in terms of Kp. NOTE: Capitalization counts. pK = %3D Submit
- You are diligently doing an assignment when a question comes up that had a pH of -1. Is this likely a typo by a tired instructor, or is this number indeed possible? Explain clearly, using an example if need.Please answer this question asap I will rate you for sure. Calculate the pH and fraction of dissociation ( ? ) for each of the acetic acid ( CH3COOH , p?a=4.756 ) solutions. A 0.00161 M solution of CH3COOH A 3.01×10−123.01×10−12 M solution of CH3COOHCH3COOH.Drive-Google X Logout Successhil X O- Mail- Mariin, And X e Kegistration-Lifer X Sign pw.com/iln/takeAssignment/takeCovalentActivity.do?locator=assignment-take Clear All (C,H3),NH, Stronger Bronsted-Lowry acid Weaker Bronsted-Lowry acid NO, (C;H3)½NH Stronger Bronsted-Lowry base HNO2 Weaker Bronsted-Lowry base Cengage Learning | Cengage Technical Support a W
- [References] This question has multiple parts. Work all the parts to get the most points. Use the References to access important values if needed for this question. The pK of a solution is defined by the equation: eq pK, = =log K, Where: K = acid dissociation constant req NOTE: Write Ka as Ka for the answers below. req a Use the rules for logarithms and exponents to solve for K. in terms of pK. K = 2req Submit 2req 2req Submit Answer Retry Entire Group 4 more group attempts remaining Previous Next Save and Exit Cengage Learning | Cengage Technical Support6. Find Ka and Kb of each of the following amphiprotic anions and determine if they act as an acid or a base in water solution. а) НРО- Ka = (С.А. 3D Kb = A or B b) HC,H;0, Ka = (C. A. = ) Kb = A or B c) HSO; Ka = : (C. A. = Kb = A or B. Give an example of a Lewis acid-base pair and a frustrated Lewis acid-base pair. What is the difference between these two systems? What is the mechanism for the reaction with H2?