QUESTION 4 If you find that you need an acid to base ratio of 4.23 and you are using 50.00mL of a 1.00M acid solution, what volume of 1.00M base solution should you use?
a) 212 mL
b) 32.6 mL
c) 85.9 mL
d) 11.8 mL
QUESTION 4 If you find that you need an acid to base ratio of 4.23 and...
QUESTION 3 To make a buffer of formic acid (Ka = 1.8 x 10-4) with a pH = 4.00, what ratio of formic acid to sodium formate is required? (Notice that I am asking for the ratio of acid to base, not base to acid!) a) 1.25 b) 0.56 c) 0.82 d) 1.87 QUESTION 4 If you find that you need an acid to base ratio of 4.23 and you are using 50.00mL of a 1.00M acid solution, what volume...
Strong base is dissolved in 765 mL of 0.400 M weak acid (Ka = 4.23 × 10-5) to make a buffer with a pH of 4.19. Assume that the volume remains constant when the base is added. Strong base is dissolved in 765 mL of 0.400 M weak acid (Ka 4.23x 10) to make a buffer with a pH of 4.19. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) → H2O()-A-(aq) Calculate the pKa...
Now we need to find the mass of base to use. What is the ratio [base]/[acid]? Target pH = 5.25 Acid/Base pair: CH,CO2H/NaCH,CO2 PK, -4.74 [NaCH3CO2]> [CH,CO2H] [CH,CO2H] = 0.100 M 6.01 g CH3CO2H required [base)/(acid] = Check Next (4 of 6) Show Approach
Please answer all parts. 4. Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can "absorb five times as much acid or base as a 0.1 M buffer for a iven p calculate the new pH after a particular quantity of acid or base is ad You are given 60...
Question 4 (0.5 points) You are asked to generate 60 ml of a 10% nitric acid solution using the bottle below. Which equation should you use to determine how much of this 70% nitric acid solution you need to use to prepare this solution? DNitric acid (70%) OC1V1-C2V OM= moles/L % - solute amount (g or mls)/total volume x 100
Enter a response, and then click Su . Now we need to find the mass of base to use. What is the ratio [base][acid]? Target pH = 2.52 Acid/Base pair: H3PO4/NaH2PO4 pka = 2.12 [NaH2PO4] > [H3PO4] [H3PO4) = 0.10 M 9.80 g H3PO, required [base)(acid] =
question 2- all 4 parts. please type orwritr clearly thank you! 2. Buffer capacity refers to the amount of acid or base a buffer can "absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can "absorb" five times as much acid or base as a 0.1 M buffer for a given pH change. In this problem you begin with a buffer of known...
4- A 0.4M acid is neutralized with 10 mL of 2.8M Base solution. Find the volume of acid. 8. A solution has a PH of 4.5, find the following: POH = [H+]= [OH-]- TI --23 C P2 = 3.0 atm V2-3.6 L 9. P1 - 1140 mmHg V1 = 1800 mL T2 - ? 10- How many grams of N2O is in a 2200 mL container with a pressure of 0.75 atm and a temperature of 77 C?
Question 4 Status: Not yet answered | Points possible: 1.00 Suppose you are titrating an acid of unknown concentration with a standardized base. At the beginning of the titration, you read the base titrant volume as 2.86 mL. After running the titration and reaching the endpoint, you read the base titrant volume as 21.17 mL. What volume, in mL, of base was required for the titration? Type answer: Question 6 Status: Not yet answered Points possible: 1.00 Suppose you are...
i need to find the ratio of B- and HB to create a ph level of 11 using the pka found in part 1 and 2 of question c. what equation would i use to fibd the ratio and the volume? 5. Preparation of Buffer Target pH to be prepared pK, from C.1 and C.2 Show calculation of B)/(HB) ratio needed: Ratio [B]/[HB) needed: Volumes used to create above ratio: ml. HB ml phl of prepared buffer c. Some Properties...