Calculate the pH at 25 °C of a 0.24M solution of ammonium bromide (NH,Br). Note that ammonia (NH;) is a weak base with a p K, of 4.75 Round your answer to 1 decimal place. pH = |
Q: The Ksp of aluminum hydroxide, Al(OH)3, is 2 × 10−31. What pH is required to limit the Al3+…
A: Al(OH)3 (s) ------> Al3+ (aq) + 3 OH- (aq) The Ksp of the reaction is given by Ksp = [Al3+] X…
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A: Weak acids acidic strength can be measured by Ka value When a weak acid HA dissolved in water…
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A: Given that: The solution is an aqueous solution of pyridine, C5NH5(aq) To find: The chemical…
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Q: 2), 3), 4)
A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…
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A:
Q: The autoionization constant of water (K„) is 1.139 × 10-15 at 0°C and 9.614 × 10-14 at 60°C. (a)…
A: a) calculate the standard enthalpy of autoionization of water. Given: (Kw)1 at 0oC = 1.139×10-15…
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A: When hypobromous acid dissolved in water it gives following Equilibrium - HBrO + H2O <===>…
Q: The acid dissociation constant K, of alloxanic acid (HC,H,N,0,) is 2.24 x 10 '. Calculate the pH of…
A: Answer
Q: Consider an aqueous solution of pyridine, C5NH5(aq), with F = 5.0 mM, at 1 bar and at 298 K.…
A: According to the Bronsted-Lowry acid-base theory, an acid is that which gives H+ ions and the base…
Q: The pOH of an aqueous solution of 0.354 M acetylsalicylic acid (aspirin), HC9H7O4, is
A:
Q: 0.1 M Na2CO3 solution, using the given pH data, write expression for equilibrium constant (Ka or…
A: As the pH of Na2CO3 is 11.0 which means that it is basic in nature.
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Q: Consider the following equilibrium between propanoic acid and its conjugate base: H20: + H30+…
A: The given reaction is,
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Q: The pH of a 0.70 mol/L weak base solution is 10.22. What is the Kb of the base?
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Q: The acid dissociation constant K, of acetic acid (HCH, CO,) is 1.8× 10¯³. a Calculate the pH of a…
A: Given Ka = 1.8*10-5 [Acid] = 0.47 M To find pH the formula used pH = pKa + log[Conjugate…
Q: Determine the K of a weak base if a 0.33 M solution of the base has a pH of 12.18 at 25°C. x 10
A: Given that: concentration of weak base = 0.33 M pH = 12.18 To find: Kb?
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Q: A solution is prepared at 25 °C that is initially 0.43 M in propanoic acid (HC,H,CO,), a weak acid…
A: Given :- [HC2H5CO2] = 0.43 M [KC2H5CO2] = 0.11 M Ka for HC2H5CO2 = 1.3 × 10-5 To calculate :-…
Q: The value of K, for acetylsalicylic acid (aspirin) is 3.00x104. What is the value of Kp, for its…
A: Given: Ka value of acetylsalicylic acid = 3.00×10-4
Q: The acid dissociation constant K, of acetic acid (HCH,Co,) is 1.8 x 10. D. Calculate the pH of a…
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Q: 0.1 M NH4CI solution, using the given pH data, write expression for equilibrium constant (Ka or Kb):
A: Net ionic reaction for the hydrolysis reaction in NH4Cl is given below NH4+(aq) +…
Q: In the laboratory, a general chemistry student measured the pH of a 0.354 M aqueous solution of…
A: Given that: pH = 0.354 [C8H10N4O2] = 12.063 To find: Kb
Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 × 10¯'. Calculate the pH of a 3.3…
A:
Q: The pOH of an aqueous solution of 0.354 M nitrous acid is .
A: Given: Concentration of HNO2 = 0.354 M
Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?
A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…
Q: The acid dissociation constant K, of alloxanic acid (HC,H;N,0,) is 2.24 x 10¬'. Calculate the pH of…
A: Given, Ka = 2.24×10-7 The value of Ka is very low. So for a weak acid,
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Q: Write the formula for the conjugate acid of each of the following bases: (a) HS¯, (b) HCO,, (c)…
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Q: LAI 298 15 K, the acid dissociation constant, Aas for propanoic acid, CH3CH,COOH, is 1.35 x 10 Write…
A: Propanoic acid is a weak acid, it does not dissociate completely.
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Q: What is the pH of a 0.248 M aqueous solution of potasslum acetate, KCH,CO0 at 25 °C? (K, for CH,COOH…
A: 1.) Potassium acetate is a salt of conjugate base of acetic acid. So we would draw ICE table and use…
Q: The acid dissociation constant K, of alloxanic acid (HC,H,N,0,) is 2.24 × 10 '. Calculate the pH of…
A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Determine the pH of a 0.13 M acetic acid solution. The K, of acetic acid is 1.8 X 10 5.
A:
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A: The to the following question is-
Q: A solution is prepared at 25 °C that is initially 0.34M in acetic acid (HCH,CO,), a weak acid with…
A:
Q: The pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar…
A: The relationship between pH and H+ ion concentration is: pH=-logH+ Given: pH of an aqueous solution…
Q: Nitrous acid, HNO2 (aq) has a Ka value of 4.0 x 10-4. What is the pH and POH of a 0.0500 M solution…
A: The question is based on the concept of equilibrium. we have to determine PH and pOH of weak acid…
Q: [ОН ] pH pH pH Calculated раper meter pH 1. 0.1 M 2. 0.01 M 3. 0.001 M 4. 0.0001 M [H,O° ] pH pH…
A: Given that : We have to calculate the pH for the given concentrations of [H3O+] and [OH-] ions.
Q: Calculate the pOH value of a 0.0150 M solution of pyridine, C5H5N.
A:
Q: The acid dissociation constant K, of hypobromous acid (HB1O) is 2.3 × 10 Calculate the pH of a 2.0 M…
A: Given: [HBrO] = 2.0 M Ka = 2.3×10-9 The hypobromous acid, HBrO is a weak monoprotic acid,…
Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 × 10¬1º. Calculate the pH of a…
A: Given, initial concentration of HCN = 3.0 M Ka for HCN = 6.2 x 10-10 The hydrocyanic acid…
Q: A solution is prepared at 25 °C that is initially 0.28M in propanoic acid (HC,H,Co,), a weak acid…
A:
Q: Construct the expression for Ka for the weak acid, CH,COOH. CH,COOH(aq) + H,O(1) = H,0*(aq) +…
A: Expression of Ka The equilibrium constant expression is the ratio of the concentrations of a…
Q: The value of K, for acetylsalicylic acid (aspirin) is 3.00x104. What is the value of Kp, for its…
A: Ans. 3.33*10-11
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- The pH of an aqueous solution of pyridine (C5H5N) is 10.0 at room temperature. What is the initial molar concentration of C5H5N, if its base ionization constant is: Kb = 1.7×10–9?Calculate the pH and pOH of a solution resulting from dissolving 0.75 grams of perchloric acid in enough water to obtain a final solution of 1500 mL. Take into account that for each mole of perchloric acid it dissociates in the aqueous medium, releasing 1 mole of hydrogen ions.How do I calculate pH of a salt? for example in 0.10 M NaClO4(aq)?
- Calculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in 95.5 mL of 0.10 M acetic acid, CH3 COOH(aq). Assume the volume change upon dissolving the sodium is negligible. Ka of CH3COOH is 1.75 x 10-5.8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C. (b) For the reaction A(g) =A(l), the equilibrium constant is 0.666 at 25.0 ◦C and 0.222 at 75.0 ◦C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?The pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar concentration of CH3COOH, if its acid ionization constant is Ka = 1.8×10–5?
- Determine the base ionization constant (in x 10^5) of a 0.0925 g sample of week base (molar mass = 17.03 g/mol), B, that is dissolved in water to produce 100 mL of a solution with a pH of 11.00.What is the concentration of hydroxide ion in a 0.45 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0 ✕ 10−14.) M What is the pH?Acidic water can be treated with basic substances to increase the pH, although such a procedure is usually only a temporary cure. Calculate the minimum mass of lime, CaO, needed to adjust the pH of a small lake 1V = 4 * 109 L2 from 5.0 to 6.5. Why might more lime be needed?
- Consider an aqueous solution of 0.40 M phenol. If you add HCl to the phenol solution until the pH reaches 3.70, what will be the ratio of phenolate (the conjugate base of phenol) to phenol? Assume that the Ka for phenol is 1.0 x 10^-10.Calculate the pOH value of a 0.0150 M solution of pyridine, C5H5N.Calculate the pH of a solution prepared by dissolving 1.75 g of sodium acetate, CH3COON,, in 53.5 mL of 0.15 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5.