Using the Cr value from the below graph find the concentrations of [HCO3], [CO3], [OH‍], a [H*] at pH 7.5 and 11 by both from graph (no need to draw the graph) and from equations 2 2 IH, Co 17 3 4 8 -log concentration, DC 9 5 BD 10 11H 12 IHCO, 1 LO PH 7 8 90 10 11 12 13 14 IHCO, 1 (OH IH'I (00-1 IH, CO

Using the Cr value from the below graph find the concentrations of [HCO3], [CO3], [OH‍], a [H*] at pH 7.5 and 11 by both from graph (no need to draw the graph) and from equations 2 2 IH, Co 17 3 4 8 -log concentration, DC 9 5 BD 10 11H 12 IHCO, 1 LO PH 7 8 90 10 11 12 13 14 IHCO, 1 (OH IH'I (00-1 IH, CO

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...

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#6 pH and pOH calculations 1. Determine the pH, pOH, [H], and [OH-] for each of the following problems. You may assume each acid and base listed will 100% dissociate. a. 8.50 x 10-³ M HBr b. 5.00 mL of 0.250M HCIO4 diluted to 50.0 mL (M₁V₁ = M₂V₂) c. 1.52g of HNO3 in 575 mL of solution. Be sure to convert to molarity. d. 1.50 x 10-³ M Sr(OH)2 solution e. 2.250 g of LiOH dissolved in 250.0 mL of solution. Be sure to convert to molarity.
1. For each of the solutions in part 3, calculate an expected pH. The Ka for HC₂H3O2 is: 1.8 x 10¹5 and the Kb for NH3 is 1.76 x 10. Remember to account for the dilution factor. a. 10.0mL of 0.10 M HC₂H₂O2 + 5.0mL of 0.10M HCI b. 10.0mL of 0.10M NH₂ + 5.0mL of 0.10M NaOH c. 10.0mL of 0.10M HC₂H₂O₂ +10.0mL 0.10M NaC₂H₂O₂ d. 10.0mL of 0.10 M NH3 + 10.0mL of 0.10M NH₂CI 2. Which solution(s) in question 1 would be considered a buffer solution? 3. Complete the calculation for K, from the earlier discussion of the amphoteric salt. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution. (1) H₂PO4 (aq) + H₂O → H3O*(aq) + HPO42(aq); Ka2 = 6.2 x 10-8 (2) H₂PO4 (aq) + H₂O → Kw H3PO4(aq) + OH(aq); Kb = ??? Kal 4. Similarly, the HPO4 ion is also amphoteric. The two possible reactions are: (1) HPO4² (aq) + H₂O → H3O*(aq) + PO4³(aq); Kas = 4.2 x 10-¹3 (2) HPO4 (aq) + H₂O Kw → H₂PO4 (aq) + OH(aq); Kb = <= ??? K₁2 Complete the calculation for Kb. Will this ion be acidic or…
Remaining Time: 53 minutes, 34 seconds. > Question Completion Status: D) 1× 10²M QUESTION 15 What is the pH of a solution with [H3O+] = 1 × M? A) 9.0 OB)-9.0 OC) 5.0 ⒸD) -5.0 QUESTION 16 The [H3O*] of a solution with pH = 2.0 is 7
Calculations: pH= -log [H3O+] pOH= log [OH-] [H3O+]=10-ph [OH-]= 10-ph pH+pOH=14.00 Kw= [H3O+][OH-]=1.0x10-14 **Need help with the two left rows, that are blank, using the calculations mentioned above**
Solutions for question 1 please
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16:03 Sun Mar 28 Done < AA A session.masteringchemistry.com
1. What is the pH of a solution of 20.0 mL of 2 M KOH with 20mL of 2 M HF? (ka = 7.2e-4 and kb = 1.4e -11) 2. What is the pH of a solution of 20.0mL of 2 M HF with 60 mL of 2 M KOH? (ka = 7.2e-4) and kb = 1.4e -11)
ISSED THIS? Read Section 17.9. You can click on the Review link access the section in your eText. alculate [H3O+] and the pH of each H2SO4 solution Ka2 = 0.012). At approximately what concentration does the x is mall approximation break down? Calculate [H3O+] for a 0.45 M solution. Express your answer in molarity to two significant figures. [H3O+] = ΜΕ ΑΣΦ Submit Request Answer Part B Complete previous part(s) Part C Calculate [H3O+] for a 0.10 M solution. Express your answer in molarity to two significant figures. [H3O+] = 1 ΕΠΙ ΑΣΦ Submit Previous Answers Request Answer × Incorrect; Try Again; 9 attempts remaining Part D Complete previous part(s) Part E Calculate [H3O+] for a 0.041 M solution. M M B Re
Q 36.
3. Determine if NaHCO, is acidic, basic, or neutral by comparing the Ka & Kb of the amphiprotic species. (H,CO, Ka, = 4.3x107, Ka, = 4.8x101"1)