
Can you explain why? Question 5 0/2 pts Which combination would make the MOST effective buffer...
Can you explain step by step why this is so?
Question 5 0/2 pts Which combination would make the MOST effective buffer solution? Correct Answer 0.1 M H2CO3 and 1.0 M NaHCO3 0.1 M H2CO3 and 2.0 M NaHCO3 0.15 MH2CO3 and 0.015 M NaHCO3 You Answered 0.1 MH2CO3 and 0.1 M NaHCO3
Which of the following solutions would have the lowest buffer capacity? 0.10 M H2CO3, 0.15 M NaHCO3 2.0 MHC2H302, 2.0 M KC2H302 1.0 M HCOOH, 1.15 M NaHCOO 0.50 MH3PO4, 0.35 M KH2PO4
please explain how you got these answers!!
and me 17) (5 pts) Calculate the pH of a solution that is 0.15 Min ammonia (NH3) and 0.40 ammonium chloride, given the ionization constant of the base, kb, NH3 = 1.76 X 10 equilibrium reaction: NH3(aq) + H20 (1) 2 NH4(aq) + OH' (aq) A) 5.18 B) 8.82 C) 9.25 D) 9.50 E) 9.63 18) (5 pts) By far the most important buffer for maintaining acid-base balance in the blood is the...
Which mass of which salt below should be dissolved in 0.20 M H2CO3 (Ka = 4.2*10-7) to make 500 mL of an appropriate buffer solution with pH = 5.76? (Assume constant volume during dissolution). a) 4.0 g NaHCO3 b) 8.0 g NaHCO3 c) 2.0 g NaHCO3 d) 5.1 g Na2CO3 e) 2.6 g Na2CO3 I know the answer is C. Can someone please explain how to get this answer, and please explain why it would be NaHCO3 instead of Na2CO3?...
63. You need to make a pH 10.70 buffer solution starting with 5.0 L of 2.0 M NaHCO3. You have a 2.0 L bottle of concentrated HCI (11.65 M) and 500 g bottle of solid sodium hydroxide. Show your calculations and appropriate chemical reactions to explain how you would convert the 5.0 L of 2.0 M NaHCO3 to a buffer with pH of 10.70.
Question 14 3 pts Which of the following pairs would be appropriate to make a buffer of PH 2.0? O HNO2 and KNO2 O NaHSO4 and H2SO4 Na2SO3 and NaHSO3 Na2HPO4 and Na3PO4 O H2C204 and NaHC204 3 pts Question 15 Which of the following pairs will make a buffer? Question 3 3 pts What is the solubility of SrF2 (s) in moles per liter (mol/L) in pure water? O 3.7 x 10-5 O 5.3 x 105 O 2.8 x...
6+ (20 pts.) You prepare a buffer by ading 0.I mol of Na,PO, and 0.15 mol of NaJHPO, to 1.0 L of water. (pKal-2.148, pk, 7.198, and pKas 12.375) a. What do you expect the pH to be? b. If instead you begin with 1.0 L of a 0.1 M solution of NaH2POs, how many ml of a 0.5 M KOH solution do you need to add in order to reach a pH of 9.5?
For each of the weak acids listed below, consider how you would make a buffer solution where the weak acid has a concentration of 0.5 M at equilibrium. Determine what molarity for each potassium conjugate base salt would need to be added to make 500 mL of an effective buffer with a pH of 5.32. Which acid would make the best buffer at this pH? Which conjugate base salt would be the most economical (cheapest) out of the three choices? ...
Select any of the following combinations which would make a good buffer solution? 0.3 M NH C1 + 0.1 M HCI 0 0.1 M HCN + 0.2 M NaCN 0.2 M NH3 + 0.1 M NH4Br 0.3 M HC2H302 +0.1 M HCI 0.05 M KC2H302 0.2 M NaF + 0.2 M NaOH 0.5 M HI + 0.5 M RbI 0.05 M HC2H302 (acetic acid) + 0.05 M KC2H302 0.3 M NaNO3 + 0.2 M NaOH 0.05 M H2CO3 + 0.05...
Select any of the following combinations which would make a good buffer solution? O 0.3 M HC2H302 + 0.1 M HCI 0.05 M H2CO3 + 0.05 M KHCO3 0.05 M KC2H302 0 0.1 M HCN + 0.2 M NaCN 0.2 M NaF + 0.2 M NaOH O 0.3 M NH4CI O 0.2 M NH3 + 0.1 M NH4Br O 0.3 M NH4Cl + 0.1 M HCI O 0.3 M NH4Cl + 0.1 M NH3 O 0.5 M HI + 0.5...