Help pls with all of these Acids/Bases & pH Worksheet (continued)Complete the following table by filling in the empty spaces. Indicate if the solution is acidic, basic or neutral.You should be able to do the starred (*) items without a calculator. (Problem #23-34)[HO)[OH]pHРОНAcidic/Basic/Neutral2.35 x 104.2553x10-122-62911-37acidic1.0284x10-74.93 x 106-69287* 307acidic4.775x10-90*3218.3205*670basic10.270103.72 x 10*1.00 x 102.5805.260*1.00 x 104.27 x 10*8.0002.040Complete the following problems which require more than a single step. SHOW YOUR WORK & STEPS35. Given a solution with a hydroxide ion concentration, [OH] = 2.73 x 10, what is the pH?

Answered: Image /qna-images/answer/b5430ae4-7917-4db4-9dad-f1935c35fce7.jpg

Complete the following table by filling in the empty spaces. Indicate if the solution is acidic, basic or neutral. You should be able to do the starred (*) items without a calculator. (Problem #23-34) [HO) [OH] PH РОН Acidic/Basic/Neutral 4.2553x10-12 2.35 x 103 2-629 acidic 11-37 10284x10-7 4.93 x 10 8 6-6928 7* 307 acidic 4.775x10-9 0*321 8.320 5*670 basic 10.270 10 3.72 x 10 *1.00 x 10 2.580

Complete the following table by filling in the empty spaces. Indicate if the solution is acidic, basic or neutral. You should be able to do the starred () items without a calculator. (Problem #23-34) [HO) [OH] PH РОН Acidic/Basic/Neutral 4.2553x10-12 2.35 x 103 2-629 acidic 11-37 10284x10-7 4.93 x 10 8 6-6928 7 307 acidic 4.775x10-9 0321 8.320 5670 basic 10.270 10 3.72 x 10 *1.00 x 10 2.580

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter16: Amines

Section: Chapter Questions

Problem 16.27P: 16-27 Guanidine, p/Ca 13.6, is a very strong base, almost as basic as hydroxide ion. NH NH2+ II II...

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16-27 Guanidine, p/Ca 13.6, is a very strong base, almost as basic as hydroxide ion. NH NH2+ II II H2N—C—NH2 + H2O H2N—C—NH2 + OH" Guanidine Guanidinium ion pKb = 13.6 Complete the Lewis structure for guanidine, showing all valence electrons. The remarkable basicity of guanidine is attributed to the fact that the positive charge on the guanidinium ion is delocalized by resonance over the three nitrogen atoms. This delocalization increases the stability of the guanidinium ion relative to the ammonium ion or substituted ammonium ions. Draw three equivalent contributing structures for the guanidinium ion and show by the use of curved arrows how these three contributors are related. Propose an explanation for the fact that protonation occurs on the C=NH nitrogen rather than on one of the —NH., nitrogens. (Hint: Consider the resonance stabilization of the structure formed by protonation on a —NH., nitrogen compared with the resonance stabilization of the structure formed by protonation on the =NH nitrogen.) Predict the N—C—N bond angles in the hybrid. Which is the stronger acid, the ammonium ion or the guanidinium ion?
(a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.
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?
Complete the following table "predicted pH." Please show all work on a separate sheet of paper and attach. Note that the pK, of H₂PO4 is 7.2. Actual pH Predicted pH Original After 45 µL of 5 M NaOH solution 4.30 6.05 After 205 μL more of 5M NaOH 6.90 After 205 μL more of 5M NaOH 11.01 After 45 μL more of 5 M NaOH 11.29
pH pOH [H*] [OH'] acid or 2.41 10-6 gs for all answers) US VI 11:41 Cbp esc #3 24 & back
Q8 (a) Based from the following reaction: H-ci: H. H. + (i) Determine the conjugate acid and conjugate base. (ii) Show the mechanism of the deprotonation reaction occurs using arrows.
I Normal 1 No Spac.. Heading 1 Heading 2 Title Styles Paragraph 5. Fill in the following table: [H3O"] РОН [OH'] ACID or BASE pH 7.21 9.84 x 10° M 3.25 2.64 x 102 M 2.49
[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 Support
SHOW WORK. Perform the following calculations & determinations for this solution. 6.84 x 10 2 M OH Calculate the molarity of H. Enter the value in the first blank (with proper sig figs) and the exponent with proper sign in the second blank. x 10 M. Calculate the pH for this solution and report the result 5 2 decimal places. pH: Is this solution acidic, basic, or neutral? Enter the term that applies. Relative acidity:
Q4) What are some real-world applications in which pH is an important factor? Please list your citations.
Correction: pH=-log[H+] * Chemistry. The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per liter, in the solution, which means that it is a measure of the acidity or basicity of the solution. The letters pH stand for "power of hydrogen", and the numerical value as defined as pH = Very acid corresponds to pH values near 1, Neutral corresponds to a pH near 7 (pure water), and Very basic corresponds to values near 14. If the wine has an approximate hydrogen ion concentration of 5.01×104 , calculate its pH value.
2- 3C₂² 1 Write the acidic equilibrium equation for CCI₂HCOOH. Be sure to include the proper phases for all species within the reaction. + 2 (s) H₂O ap here or pull up for additional resources 3 H ( Reset 4 (1) Question 62 of 75 O LO 5 ) 6 x H₂O CI 7 (g) 8 OH 9 12 (aq) C X 0 LTE 23% Submit