Attempt 3 NH, is a weak base (K, = 1.8 x 10) and so the salt NH,Cl acts as a weak acid. What is the pH of a solution that is 0.038 M in NH,Cl at 25 °C? pH =
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Q: 1.80
A: Dear student I have given answer to your question in the image format.
Q: Part A What is the H+ concentration for an aqueous solution with pOH= 4.47 at 25 °C? Express your…
A: Concentration of H+ can be calculated as follows
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Q: B: What is the pH of 0.6 M NH,Cl solution? Discuss your results. (K of NH= 1.8 x 10 NH4+ + H2O+→…
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Q: B: What is the pH of 0.6 M NH.CI solution? Discuss your results. (K of NH= 1.8 x 105) NH. + H2O+ H3O…
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Q: PARTICIPATION op Which acid is stronger: HF (Ka=6.4x10“ ) or NH,*(Kb for NH, is 1.8x10*)?
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Dissociation constant of base is given by
The Ka is calculated as
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- For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)What is the pH of a solution obtained by adding 13.0 g of NaOH to 795 mL of a 0.200 M solution of Sr(OH)2? Assume no volume change after NaOH is added.The pH of a solution of Ba(OH)2 is 10.66 at 25 . What is the hydroxide ion concentration in the solution? If the solution volume is 125 mL, what mass of Ba(OH)2 must have been dissolved?
- The ion HTe- is an amphiprotic species; it can act as either an acid or a base.. (a) What is Ka for the acid reaction of HTe- with H2O?. (b) What is Kb, for the reaction in which HTe- functions as a base in water?. (c) Demonstrate whether or not the second ionization of H2Te can be neglected in the calculation of [HTe-] in a 0.10 M solution of H2Te.NH3 is a weak base (Kb = in NH4Cl at 25 °C? pH = x10 TOOLS 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.046 MNH, is a weak base (K, = 1.8 x 10) and so the salt NH,Cl acts as a weak acid. What is the pH of a solution that is 0.046 M in NHCI at 25 °C? pH =
- Ascorbic acid (H,C, H,0,) is a diprotic acid. The acid dissocation constants for H,C. H,O, are K - 800 x 10 and Ka- 1.60 x 10-1 Determine the pH of a 0.138 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. (H,C,H,0, = M |HC, H,0;] - C,H,O-CH, NH, is a weak base (K, = 5.0 x 1o4), so the salt CH,NH,NO, acts as a weak acid. What is the pH of a solution that is 0.0590 M in CH,NH,NO, at 25 °C? pH =Sodium nitride (NaNO2) is often used as a preservative for meats.a) Knowing that the Ka of nitrous acid (HNO2) is 4.52 x 10-4, find the concentration of OH-, the concentration of [H3O+] and the pH of a nitride solution sodium (NaNO2) 0.150 M. (Reminder: the nitride ion, NO2-, is the conjugate base of nitrous acid) b) What amount (in mol) of sodium nitrite (NaNO2) needs to be added to 100.0 mL of 0.150 M nitrous acid (HNO2) in order to prepare a buffer solution with a pH of 3.50?
- NH3 is a weak base (K₁ = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.036 M in NH4Cl at 25 °C? pH =predicting the qualitative acid-base properties of salts Consider the following data on some weak acids and weak bases: name acetic acid acid hydrocyanic acid solution 0.1 M NaCN 0.1 M NH C 0.1 MHONH,Br Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a 2 next to the solution that will have the next lowest pH, and so on. 0.1 M KCH₂CO₂ K₁ formula HCH,CO₂ 1.8x10 HCN 4.9 × 10 10 pH choose one X Ű choose one choose one choose one base 3 Ċ K₂ name formula ammonia NH₂ 1.8×10 hydroxylamine HONH₂ 1.1×108What is the pH of a solution of 0.400 M CH,NH, containing 0.100 M CH,NH,1? (Kb of CH,NH, is 4.4 x 104)