sub= 18 help 12Solution[H3O°]calculatedpHSolutionpH[H3O*]calculatedBoiled (but cooled)6.18Boiled (but cooled) H20H20+ 1 drop of 1M HCIn.+ 1 drop of 1M NaOH3.473.02S.+ 2 drops of 1M HCIO.t.+ 2 drops of 1M NAOH8.969.601.46р.+ 3 drops of 1M HCI2. 19+ 3 drops of 1M NAOHu.q.+ 4 drops of 1M HCIV.+ 4 drops of 1M NAOH2,54r.+ 5 drops of 1M HCI2,36w.+ 5 drops of 1M NaOH10.08Part D Buffer pH (Weak Acid and Its Salt)(report three sig Fig)SolutionpH MeterpH calculatedPK,10.5 M Acetic Acid?*CH3COOH3-23?*20.5 M CH3COONA5.713mixture 3?**4.994mixture 44.93?**5.23mixture 5?**6Mixture 6?****Calculate pH using a formula (ref. textbook) that relates pH and PK, for buffer

PH = -log [H3O+] Where [H3O+] = concentration of H3O+ Then [H3O+] = 10-PH

Solution pH [H3O'] Solution [H30*] calculated pH calculated Boiled (but cooled) Boiled (but cooled) H2O 6.18 3. 47 3.02 618 H20 + 1 drop of 1M HCI n. + 1 drop of 1M NaOH S. O. + 2 drops of 1M HCI + 2 drops of 1M NAOH 8.96 9.60 1.46 10.09 p. + 3 drops of 1M HCI 2.19 u. + 3 drops of 1M NaOH q. + 4 drops of 1M HCI 2,56 + 4 drops of 1M NaOH V. + 5 drops of 1M HCI г. 2,36 w. + 5 drops of 1M NAOH t.

Solution pH [H3O'] Solution [H30*] calculated pH calculated Boiled (but cooled) Boiled (but cooled) H2O 6.18 3. 47 3.02 618 H20 + 1 drop of 1M HCI n. + 1 drop of 1M NaOH S. O. + 2 drops of 1M HCI + 2 drops of 1M NAOH 8.96 9.60 1.46 10.09 p. + 3 drops of 1M HCI 2.19 u. + 3 drops of 1M NaOH q. + 4 drops of 1M HCI 2,56 + 4 drops of 1M NaOH V. + 5 drops of 1M HCI г. 2,36 w. + 5 drops of 1M NAOH t.

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter13: Fundamental Equilibrium Concepts

Section: Chapter Questions

Problem 13E: For a titration to be effective, the reaction must be rapid and the yield of the reaction must...

See similar textbooks

Similar questions

Identify the correct equation for the equilibrium constant K, for the weak acid dissociation of acetic acid. HC,H;O, (aq) + H,0 (1) H;0+ (aq) + C,H;O,¯ (aq) Select one: [H,O*|[C,H,0, [HC,H3O2|[H2O] HC,H,O,] [H,O"|C,H,0, K. K. [HC,H;O2|[H2O) [H;O*|[CH,O2 K = O Ka = [H,O*|[C,H,0,) [HC;H,O2]
H2O(l) + H2O(l) (double- headed arrow) H3O+(aq) + OH-(aq) At 5.0o C, the value of Kw for the equilibrium shown above is 1.9 x 10-15 and the value of pKw is 14.73. Based on this information, which of the following is correct for pure water at this temperature. A) H3O+ = sqrt( 1.9 x 10-15 ) B) pH = -log( 1.9x 10-15) C) 14.73 =( H3O+)(OH-) D) pOH = pH + 14.73
The dissociation of the weak acid acetic acid (CH3COOH) is represented by the equation below. Enter the equation including all formatting and physical states in the answer blank. CH,COOH(ag) + H,0() – H,0*(aq) +CH,Coo"(aq) x | x. Me -. 8. (agi.
5:23 O13%DE elearning.yu.edu.jo/m O A student was given 2 beakers labeled with numbers 1 and 2, each beaker contains a clear solution. Additionally, he was given two reagent bottles labeled with A and B. Now, he added reagent A to both beakers and he noticed the formation of a precipitate in beaker 2 but not in beaker 1. However, the addition of reagent B to both beakers resulted in the formation of a precipitate in beaker 1 but not in beaker 2. Based on the information, which of the following is correct? a. compound A is the limiting reactant in beaker 1. b. compound B is the limiting reactant in beaker 2. c. compound A is the limiting reactant in beaker 2. d. compound B will be the excess reactant in beaker 1. Question 2
Q4- How many grams of sodium hydroxide (M.wt-58.5) can be added to 2.5 liter of a solution mixture of 0.3M ammonia and 0.15M ammonium chloride without changing the POH by more than 1 unit? K-1.8x 10³?
Type your numerical answers in the box provided in three significant figures (e.g., 0.123). Do not report your answer in scientific notation. No need for units. If Canvas drops your last zero digit/s, it is OKAY. (e.g. 1.20 to 1.2). Consider a solution of 0.00200 M HCIO4 for numbers 22-24. Determine the following: 22. equilibrium molar concentration of H30* = M. 23. equilibrium molar concentration of CIO,4 = 24. pH =
L_{2} is considerably more soluble in CC*L_{4}(1) than it is in H_{2}*O(1) At a certain temperature, the concentration of I_{2} in its saturated aqueous solution is 1.3*10^-3* M and the equilibrium achieved when I_{2} distributes itself between H_{2}*O and CC*L{4} is 12 (aq) rightleftharpoons 1 2 (CCL 4),; K = 85.5Part A: A 12.0-mL sample of saturated I_{2}(aq) is shaken with 12.0 mL of CC*L_{4} After equilibrium is established, the two liquid layers are separated. How many milligrams of will be in the aqueous layer? I_{2}
After the neutralization reaction of 42% 0.5 mL nitric acid and 0.28M 18 mL sodium hydroxide, a temperature increase of 15 ° C was observed and the temperature value was determined as 825 cal. According to these results; What is the number of moles of neutralized base? (d(HNO3) = 1,51 g/mL; M(HNO3)=63,01 g/mol)
Type your numerical answers in the box provided in three significant figures (e.g., 0.123). Do not report your answer in scientific notation. No need for units. If Canvas drops your last zero digit/s, it is OKAY. (e.g. 1.20 to 1.2). Consider a solution of 0.00500 M HBr for numbers 22-24. Determine the following: 22. equilibrium molar concentration of H3O = M. M. 23. equilibrium molar concentration of Br = %3D 24. pH =
g -. Use this information to calculate K., for BaCrO. L The solubility of BaCrO, in water at 25 °C is measured to be 0.0037 sp Round your answer to 2 significant digits. x10
A 1.00 liter solution contains 0.60 moles nitrous acid and 0.46 moles potassium nitrite .If 0.23 moles of perchloric acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of HNO2 will increase. B. The number of moles of NO2- will remain the same. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase.
10-18. (a) Calculate the quotient [H,PO4]/[H,PO] in 0.050 0 M KH,PO4. o no (b) Find the same quotient for 0.050 0 M K,HPO4.