Assuming that base (B:) and acid (AH) are mixed in equal concentrations and using pKa values of acid AH 3.5 and pka value of conjugate acid for the base BH 5.5 calculate what percent of BH will appear in this reaction once the equilibrium is reached. Answer is numerical. Round the answer to the nearest whole number. Don't write % symbol in the answer.

Assuming that base (B:) and acid (AH) are mixed in equal concentrations and using pKa values of acid AH 3.5 and pka value of conjugate acid for the base BH 5.5 calculate what percent of BH will appear in this reaction once the equilibrium is reached. Answer is numerical. Round the answer to the nearest whole number. Don't write % symbol in the answer.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The conjugate base that is produced after the first ionization step of carbonic acid when it has reacted with ethyl amine (CH3CH2NH2) would be _________. H2CO3 CH3CH2NH3+ HCO3- CO3-2 CH2CH2NH Given a Ksp of 4.96 X 10-9 for limestone (calcium carbonate), the calcium concentration in a limestone solution will be__________ the Ksp. greater than less than the same as cannot be determined
Calculate the concentrations of the weak acid and conjugate base for the best possible buffer at pH 3.50 knowing that the concentration of the more concentrated species between the two will be 0.2 M. Choose the buffer system you think would be best between the following three. You will need to look up literature values for the Ka/pKa on your own. Remember that a strong buffer has similar concentrations of the buffering components. Formic acid/formate Acetic acid/acetate Hypobromous acid/Hypobromite
Learning Goal: Another way to express acid strength is by using pk To understand the relation between the strength of an acid or a base and its pK, and pK, values. The degree to which a weak acid dissociates in solution is given by its acid-ionization constant, K. For the generic weak acid. HA. pk. = log K. Another way to express base strength is by using pk log K HA(ag) A (aq) + H'(aq) and the acid-ionization constant is given by Part A IA H HA K. Similarty, the degree to which a weak base reacts with HO in solution is given by its base-ionization constant, K. For the generic weak base, B. A new potential heart medicine, code named X-281, is being tested by a pharmaceutical company. Pharma pill. As a research technician at Pharma-pil you are told that X-281 is a monoprotic weak acid, but because of security concerns, the actual chemical formula must remain top secret. The company is Interested in the drug's K, value because only the dissociated form of the chemical is active in…
Phenol red is a common acid-base indicator. It has a pKa equal to 8.000. It's undissociated form is yellow and its anionic form is violet. What color would a solution containing phenol red solution if the pH is 7.50? yellow yellow-orange red-orange red-violet violet
If to 100 ml of a solution of CH3COOH with a concentration of 0.0928 N. a) 200 ml of distilled water was added. Determine its new concentration expressed to 4 decimal places, and determine the pH of the final solution. Data: pKa = 4.756 at 25°C. Consider that degree of dissociation is very small. b) If it is mixed with 100 ml of a 0.0989 N CH3COONa solution. What is the pH of the buffer solution.
Weak Acids and Buffers Write out the simple equilibrium of a weak acid (HA), labeling the conjugate acid and the conjugate base. ● Write out the Henderson-Hasselbalch equation and use this expression to define the meaning of the characteristic pką value.
Determine the Kb for a base by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 1 2 NEXT > The pH for a 0.0160 M solution of CH:CH.NH: is 8.600. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. CH:CsH&NH:(aq)+ H:O(1) OH-(aq) +CH:CeH&NH;*(aq) Initial (M) |Change (M) Equilibrium (M) 5 RESET 0.0160 8.60 -8.60 0.93 -0.93 2.50 x 109 -2.50 x 109 3.98 x 10 -3.98 х 10° 5.4 -5.4
Complete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits. acid B C Ka M 0 7.28 x 10 pK 1.17 11.3 0 relative strength (Choose one) ✓ (Choose one) ✓ (Choose one) ✓ O *10 X ?
Provide your view on this? Strong bases have weak conjugate acids with high pKa values, usually > 12.
it is stated that alkyl halides (such as n-butyl bromide, sec-butyl bromide, tert-butyl chloride, benzyl chloride, and bromobenzene) make a carbocation and the halide, before the halide reacts with the silver.(1% ethanolic silver nitrate solution) Explain why this is wrong and the actual role of the Ag+ ion as a Lewis acid
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data. Method 1-TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint. Method 2 - pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8. A. Calculate the molarity of the acid using the titration data. B. If we assume that the titrated unknown is a strong acid, predict the pH of the sample. C.…
Solve correctly please.