please answer 1 and both parts of 2
please answer 1 and both parts of 2 1. Which one of the following sets of...
both 5 and 6 please 5) What is the H30* concentration to the correct number of significant figures for solutions with the following pH values? (a) 0.00 (b) 7.00 (c) 2.63 (d) -0.42 (e) 11.21 6) (a) Calculate the pH of a buffer solution that is 0.45 M in NH4Cl and 0.15 M in NH3. (b) How would you prepare an NHACI-NH3 buffer that has a pH of 9.00? (The K. for NH3 is 1.8 x 10)
Which one of the following sets of compounds is not characteristic of a buffer? OCH3CO2H with NaCH3CO2 O NaH2PO4 with Na2HPO4 O NH3 with NH4Cl O HNO3 with NaNO3
Buffers 1. Indicate which of the following pairs of compounds could be used to make a buffer solution by placing an X in the appropriate column. Buffer Solution | Not a Buffer Solution Pair of Compounds HF and Cl H.COs and OH HNO2 and NO NHa and NH L 2. Write out the reaction of acetic acid CH.COOH reacting with water. 3. What is the pH of a buffer solution in which the (CH3COOH) is 0.229 M and the (CH...
All of the following are acid-base conjugate pairs EXCEPT Group of answer choices H2O, H3O+ NH4+, NH3 CH3COOH, CH3COO- H3O+, OH- HPO42-, PO43- The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31. What is the Ka of the acid? Group of answer choices 4.7 x 10-5 4.1 x 10-7 3.4 x 105 2.4 x 10-4 1.3 x 10-5 You have 250.0 mL of a 0.56 M solution of NaCH3COO. How many milliliters of a 0.50...
10. Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8? A) CHCO02Na / CH3COOH (Ka 1.8 x 10) NH3/NH4CI (K-5.6 x 10-10) в) NaOCl/HOCI (K= 3.2 x 10-) C) NaNO2 / HNO2 (Ka= 4.5 x 104) D) NaCl/HCI E)
Please answer all questions correctly! i promise a thumbs up if they are right. Thanks 1. Calculate the [H*] of a solution with a pH of 10.72 a. 5.25x10-4M b. 1.91x10-11M c. 1.07x10-4M d. 5.25x10-11M 2. Arsenic has a Ka of 5.5x10-3 Calculate the pka a. 5.5x10-3 b. 11.74 c. 2.26 d. 1.82x10-12 3. Calculate the pH of a 0.0002M HCl(aq) solution a. 2.00 b. 12.00 c. 3.70 d. 10.3 4. Calculate the [OH-] at equilibrium of the following reaction...
8. What is the pH of a 5.00 x 102 M Ba(OH)2(aq) solution at room temperature? a. 1.00 b. 1.30 c. 12.02 d. 12.70 e. 13.00 9. Assuming equal concentrations of conjugate acid and base, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8? a. CH3COONa/CH3COOH (K = 1.8 x 105) b. NH/NHACI (K = 5.6 x 10-1) c. NaOCI/HOCI (Ka = 3.2 x 108) d. NaNO2/HNO2 (Ka = 4.5...
Need help with these please :) Thanks What mass of sodium hypochlorite, NaOCI (molar mass 74.5 g/mol), must be added to 250 mL of 0.60 M HCIO (hypochlorous acid, K.-3.5 x 10"), in order to produce a solution having a pH of 7.257 (Ans. ; A 25.0-mL sample of 1.00 M NH, is titrated with 0.15 M HCl. What is the pH of the solation after 15.00 mL of acid have been added to the ammonia solution? K,-1.8 x 10'(Ans,pH-...
please show work Use the data in the tables below. Show appropriate work for numerical calculations. K. values: HCI HNO3 H2SO4 HSO4"- H3PO4 HF HNO2 HCOOH strong strong strong 1.3 x 10-2 7.5 x 10 7.1 x 10+ 4.5 x 10-4 1.7 x 10+ CH3COOH CsH NH H2CO3 H2PO4 NH4+ 1.8 x 105 5.9 x 10-6 4.2 x 10-7 6.2 x 10-8 5.6 x 10-10 4.9 x 10-10 4.8 x 10-11 4.8 x 10-13 HCO3 HPO42- Ksp values: 8 CaCO3...
please answer both 1 p QUESTION 4 A 29.9 mL. sample of 0.299 M methylamine, CH3NH2, is titrated with 0.331 M hydroiodic acid, HI at 25 °C. (Kb for methylamine is 4.2 104) What is the pH at the midpoint of the titration? X a 10.318 10.623 c8.318 d. 10.714 e3.377 1 point QUESTION 5 Which of the following aqueous mixtures would make a good buffer system? 0.36 M HNO3 and 0.29 M KNO3 а. 0.35 M NH4Br and 0.37...