Calculate the Ka for a unknown acid. When the acid is dissolved in water the pH of the solution is 2.98, and the concentration of the acid is 5.61 M. (Write your answer in scientific notation) Ka
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- Question 6 of 36 Retry A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H;NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10-10. 1 2 NEXT > Let x represent the original concentration of C6H5NH3* in the water. Based on the given values, set up the ICE table in order to determine the unknown. C6H;NH2(aq) + H20(1) ОН (ад) + CgH;NH;*(aq) Initial (M) 0.50 Change (M) Equilibrium (M) -1.6 x 10 10 Incorrect, 2 attempts remaining Your Initial concentration for C,H5NH3* is incorrect. Revisit the problem statement to determine the initial concentration of acid or base. Also, make sure that your values are in the correct concentration units, not mass or moles! Your Change in concentration for C6H5NH2 is incorrect. In this problem, you should use the given pH to determine the concentration of H3O* or OH at Equilibrium as appropriate. From there, you should be able…The pH of blood is 7.4. What is the ratio (to one decimal place) of bicarbonate (conjugate base) to carbonic acid (weak acid) in the blood's buffering equilibrium? Note, the K₂ of carbonic acid is 4.27 x 10-7. Write your answer this way: # to 1 Done Clear Incorrect. The ratio is 10.7 to 1, indicating that there is 10 times more bicarbonate than carbonic acid. Enter the correct answer.Example 2What is the pH of the solution that results when 0.093 g of Mg(OH)2 Ksp = 7.1 × 10–12 is mixed with(a) 75.0 mL of 0.0500 M HCl?(b) 100.0 mL of 0.0500 M HCl?(c) 15.0 mL of 0.0500 M HCl? (d) 30.0 mL of 0.0500 M MgCl2?
- A 0.036 M solution of a weak base is 0.019% ionized. What is the pH of the solution? pH= i What is the value of K for the base? Enter in scientific notation, for example, 0.00010 would be 1.0E-4. Kb =Q1a): Arrange the following 0.10 M aqueous solutions in order of increasing PH: Caso, H,SO, NH,NO, Rb,CO, NaF (Hint: start with the one of lowest PH and put < symbol when you go to the next higher PH, and continue with this < to the highest one. No calculation is required but you need to justify your answer Q1:b) Write a formula of one salt for each and also give the name 1. contains Cs* and is Basic 2. contain perchlorate; CIO, and is neutral 3. Contain NH, and are Acidicpredicting the qualitative acid-base properties of salts Consider the following data on some weak acids and weak bases: name acetic acid acid hydrocyanic acid solution 0.1 M NaCN 0.1 M NH C 0.1 MHONH,Br Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a 2 next to the solution that will have the next lowest pH, and so on. 0.1 M KCH₂CO₂ K₁ formula HCH,CO₂ 1.8x10 HCN 4.9 × 10 10 pH choose one X Ű choose one choose one choose one base 3 Ċ K₂ name formula ammonia NH₂ 1.8×10 hydroxylamine HONH₂ 1.1×108
- What is the concentration of hydroxide ion in a 0.170 M aqueous solution of hydroxylamine, NH2OH? What is the pH? (K, = 1.1 x 10-) [OH ] = pH = Submit Answer Retry Entire Group 9 more group attempts remainingPredicting the quam Consider the following data on some weak acids and weak bases: name shift acetic acid hydrofluoric acid acid solution. 0.1 M CsHsNHBr 0.1 M NaCH3CO₂ 0.1 M NaCl 0.1 M KF Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. Explanation tab caps lock Ka formula HCH₂CO₂ 1.8 x 105 HF control Check -4 6.8 x 104 1 choose one choose one choose one ✓ choose one 1 (lowest) 2 3 4 (highest) PH Q A 1 option Z 2 K₁ ammonia NH3 NH3 1.8x10-5 pyridine CHN 1.7×10⁹ base name formula W 4 S X ► command # 3 SP H E D $ 4 C R * F 5 V © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility T MacBook Pro 80 G 6 Y B & 7 H U N 8 J 1 9 M A K ) O OWhen you determine the pH of a 0.020 M solution of a weak acid whose Ka = 6.3 x10-5, which calculation lets you determine if x could be negligible? (Which of the following applies?) (6.3x10-5/0.020) < 100 (0.020/6.3x10-5 ) > 100 (0.020/6.3x10-5) < 100 (0.020 x 100) > 100 (6.3x10-5/0.020) > 100
- Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula NH,+ CH3NH3+ CH5NH3+ CH;NH3* C;H;NH+ 1.8 × 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 Ammonia NH3 CH;NH2 CH;NH2 CH;NH, C;H;N Methylamine Ethylamine Aniline Pyridine 1.7 x 10-9 3. Compute the concentration of the weak base in Molarity (Write your answer in 4 decimal places without the unit).Using the table of the weak base below, you have chosen Ammonia as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.65 M in this salt. The desired pH of the buffer should be equal to 8.8. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula NH3 CH;NH2 C¿H5NH2 C,H;NH2 C3H;N 1.8 × 10-5 4.38 × 10-4 5.6 × 10-4 3.8 × 10-10 Ammonia Methylamine Ethylamine Aniline Pyridine NH, CH;NH;* C¿H5NH3* C¢H;NH;* C;H;NH+ 1.7 x 10-9 314. Compute the concentration of the weak base in Molarity (round off answer to 4 decimal places).In the laboratory, a general chemistry student measured the pH of a 0.559 M aqueous solution of formic acid, HCOOH to be 2.013. Use the information she obtained to determine the K₂ for this acid. K₂(experiment) =|| Submit Answer Retry Entire Group 2 more group attempts remaining