Q: Calculate the pH of Ba(OH)2 solution whose 250 cm3 of a 0.01moldm-3 solution is diluted to 500 cm3…
A: The pH of a solution can be calculated as follows: pH= 14-pOH where pOH = -logOH- To calculate…
Q: Calculate the pH at 25°C of a 0.45 M aqueous solution of oxalic acid (H2C2O4). (Ka1 and Ka2 for…
A: We have to calculate the pH value.
Q: If a buffer solution is 0.170 M in a weak base (Kb = 4.2 × 10-5) and 0.490 M in its conjugate acid,…
A: Buffer solution: It is an aqueous solution which contains a mixture of a weak base and its conjugate…
Q: What is the pH of a 0.860 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)?
A: A numerical problem based on pH concept, which is to be accomplished.
Q: What is the pH of a 1.75 M solution of KX (Kb of X is 1.22 x 10°) (Please show the final result with…
A: Answer: 9.66 Weak base can't dissociate completely, it's pOH = 1/2 (PKb - logC)
Q: Calculate the pH for a 0.015 M (HC2H3O2) acetic acid solution. The Ka is 1.8 x 10 ^-5 for acetic…
A:
Q: Calculate the [OH−] of a solution of 0.1595 M C5H5NH3F if Kb = 1.800e-9 for C5H5NH2?
A: The equilibrium constant for a reaction is expressed in terms of the ratio of the concentration of…
Q: What is the pH of a 0.1250 M CH3NH3Br? Kb for CH3NH2 is 3.70e-4.
A: Given, The pH of a 0.1250 M CH3NH3Br is : Kb for CH3NH2 is 3.70e-4.
Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…
A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…
Q: The PH of 0.0296M HA ( Ka 8.4 *10-9) plus * . . 0.1026 M NaA is 4.3 2 O 8.6 7.5 O
A: The question is based on the concept of PH calculations. we have been given a weak acid and its…
Q: What is the pH of a 0.620 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 × 10-4)?
A: HNO2 => H+ + NO2- Ka = [H+][NO2-]/[HNO2] Given, Ka = 4.5x10-4 = [H+][NO2-]/[HNO2] 4.5x10-4 =…
Q: If a buffer solution is 0.410 M in a weak acid (K, = 5.9 x 10-6) and 0.210 M in its conjugate base,…
A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…
Q: What is the pH of a 0.063 M solution of benzoic acid (Ka = 6.3 × 10-5) at 25ºC?)
A: Benzoic acid is a weak acid so it will set-up equilibrium when it reacts with water…
Q: Calculate the pH of a mixture containing 0.23 M HONH2 and 0.44 M HONH3Cl. (Kb = 1.1 × 10–8) What…
A:
Q: What is the pH of a 0.570 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)?
A:
Q: How would I find the pH of the two-component solution 0.115 M in NaCl and 9.56×10−2 M in KF?
A:
Q: Calculate the pH of a buffer solution that is 0.050 M in benzoic acid (HC7H5O2) and 0.150 M in…
A: Given: [C6H5COOH] = 0.050M [C6H5COONa] = 0.150M Ka for benzoic acid =…
Q: What is the pH of a solution that is 0.28 M in acetic acid, HC2H3O2, and 0.69 M in sodium acetate,…
A: Answer:- This question is answered by using the simple concept of calculation of pH of a solution…
Q: Calculate the pH of 0.564 M HC2H3O2 (Ka of HC2H3O2 = 1.8 x 10-5)
A:
Q: What is the equilibrium percent ionization of an initially 0.32 M solution of the monoprotic acid…
A: Given that , Initial concentration of valeric acid = 0.32 M Dissociation constant , Ka = 1.44×10-5…
Q: Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8 x 10-5.
A: Interpretation: The pH of a 0.800 M NaCH3CO2 solution is to be determined.
Q: What is the pH of a 0.0620 M solution of methylamine (CH,NH2, Kb = 4.4 × 10-4)?
A:
Q: If the Kp of a weak base is 2.5 x 10-6, what is the pH of a 0.23 M solution of this base?
A: pH + pOH = 14 For a weak base solution: [OH-] = (Kb x C)1/2 Where, C = molar concentration of weak…
Q: The base protonation constant K, of allantoin (C,H,N,O,NH,) is 9.12 × 10¯°. Calculate the pH of a…
A:
Q: pH of the mixture of 0.020 M NH3 and 0.15 M NH4Cl (Kb NH3 =1.8*10^-5
A: Recall the Henderson-Hasselbalch equation to calculate pH of buffer solution pOH=pKb +…
Q: CH;NH, is a weak base (Kp = 5.0 × 104), so the salt CH,NH,NO, acts as a weak acid. What is the pH of…
A: The pH of salt of strong acid and weak base can be calculated by using formula
Q: Determine the base ionization constant (in x 10-5) of a 0.0925 g sample of a weak base (molar mass =…
A: Given :- Mass of weak base = 0.0925 g Molar mass of weak base = 17.03 g/mol Volume of water = 100 mL…
Q: Using the systematic approach, calculate the pH and the equilibrium concentrations of ALL aqueous…
A: The salt is a conjugate acid of a weak base. By solving we'll get, x = 8.49x10-⁷ Hence Equilibrium…
Q: 3. Calculate the pH of a 0.400 M KC2H3O2 (Ka for HC2H3O2 is 1.8 x 10-5)
A: In this question we have to tell the PH of the solution.
Q: What is the pH for a weak monoprotic acid if a 0.020 M solution of the acid has a Ka of 3.28 x 10-7…
A: The H3O+ concentration for the weak acid is determined given below:
Q: The Kp of dimethylamine [(CH3)2NH] is 5.90×104 at 25°C. Calculate the pH of a 1.55x103 M solution of…
A: Given : Concentration of (CH3)2NH = 1.55 × 10-3 M Kb = 5.90 × 10-4 To calculate :- pH of…
Q: Calculate the pH of a 0.424 M aqueous solution of hydrocyanic acid (HCN, Ka = 4.0×10-10).
A: pH of the solution can be calculated by using the formula, pH = [H+]. Given data, Concentration of…
Q: Calculate the pH of a 0.100 M NaCH 3CO 2 solution. Ka for acetic acid, CH 3CO 2H, is 1.8 × 103.
A:
Q: The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a/ Determine the concentration of [OH] in the…
A:
Q: What is the pH of a 0.035 M solution of benzoic acid (Ka = 6.3 × 10-5) at 25ºC?
A: Given data, Concentration of benzoic acid = 0.035 M [C6H5COOH] = 0.035 M Ka value of benzoic…
Q: CH3NH2 is a weak base (Kb = 5.0 x 10-4 ) and so the salt CH3NH3NO3 acts as a weak acid. What is the…
A:
Q: The value of K, at 25°C for proplonic acid (CaisCOgH) is 1.34 x 10. What is the pH of a 0.02019M…
A: Answer: This question is based on the understanding of Henderson-Hasslebalch equation that we use…
Q: Calculate the pH and the concentrations of all the species present in 0.010 M of Carbonic acid…
A:
Q: Calculate pH and pOH of the: 0.5M aniline (C6H5NH2) solution (Kb= 3.8 x 10-10)
A: Given, [C6H5NH2] = 0.5 M Base dissociation constant of C6H5NH2 = 3.8 x 10-10 pH and pOH = ? Base…
Q: For a solution that is 0.50 M in NH3 (Kb =1.8 x 10-5) and 0.25 M in NH4Cl, find pH and pOH
A: The Henderson-Hasselbalch equation is given as,
Q: Equimolar solutions of HF, HCOOH and HCN at 298 K have the values of Ka as 6.8×10^-4, 1.8×10^-4 and…
A:
Q: The acid dissociation constant for acetic acid (HC2H3O2, commonly abbreviated HAc) is 1.8 x 10-5.…
A: Given, Acid dissociation constant, Ka = 1.8*10-5. Molarity of acetic acid solution = 0.10M. The…
Q: Calculate the PH of: I. A 0.5 molar solution of an unknown weak acid…
A:
Q: At a temperature of 298K the value of Ka for ethanoic acid is 1.70 * 10Smoldm3. c. Calculate the pH…
A: The given data contains, Ka of ethanoic acid =1.70×10-5moldm-3Concentration of ethanoic acid =0.350…
Q: HCIO is a weak acid (K. = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…
A:
Q: What is the pH of a 0.420 M solution of C5H,NHB (Kb of C5H,N is 1.7 × 10-9)?
A: Given:: [C5H5NHBr]=0.420 M =concentration of salt=c Kb of C5H5N = 1.7×10-9 pH=?
Q: Calculate the pH and [H3O+] of a solutio n prepared by dissolving 0.25 mol of NaC2H3O2 in 500. mL of…
A: For a buffer solution: pH = pKa + log[salt]/[acid]
Q: Calculate the pH of a solution that is 0.155 M in acetic acid and 0.255 M in sodium acetate. The Ka…
A: Mixture of CH3COOH + CH3COONa is an example of acidic buffer To find its pH, use Henderson's…
Q: A solution is prepared at 25 °C that is initially 0.28M in propanoic acid (HC,H,Co,), a weak acid…
A:
Q: What is the concentration of hydroxide ions in pure water at 30.0∘C, if Kw at this temperature is…
A: The ionization of water is represented as,
Calculate the pH of a solution of 0.1421 M KCH2ClCO2 if Ka = 1.400e-3 for CH2ClCO2H?
Step by step
Solved in 2 steps with 1 images
- COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…Determine the pH of (a) A 0.10 M CH3COOH solution (ICE) (b) A solution that is 0.10 M CH3COOH and 0.10 M CH3COONa. Ka for CH3COOH = 1.8 X 10-5.What is the pH of a 0.1250 M CH3NH3Br? Kb for CH3NH2 is 3.70e-4.
- Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.Propanoic acid, CH₂CH₂COOH, is a weak monoprotic acid that is used to inhibit mould formation in bread. A student prepared a 0.10 mol/L solution of propanoic acid and found that the pH was 2.96. What is the acid dissociation constant for propanoic acid? [Hint: Setup an I.C.E. table] CH3CH₂COOH (aq) Ka for propanoic acid is: ←CH3CH₂COO (aq) + H (aq)5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5
- If the pH of a 0.200 M solution of the CICH2O¯ ion is 12.05, then what is the value for the basicity constant, Kp, of CICH20-? You do not need to make a simplifying assumption CICH,0-(aq) + H2O(1) СICH-OОH(aq) + ОН (аq) K½ = ?9) What will be the pH (aq., 25 oC) of 100.0 mL of a solution of 1.50 M C2H5NH3Br and 1.25 M C2H5NH2, after 2.00 mL of 10.00 M HCl has been added to it? Kb C2H5NH2 = 5.6 x 10–4Given that Ka's for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 x 10-4 and 5.4 x 10-10, respectively, calculate the pH of the following solutions: (a) The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3). (b) The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.
- The acid dissociation constants for sulfurous acid are: Ka = 1.2 x 10-2 and Kaz = 6.6 x 10-8. (i) Calculate the pH of a solution of 0.100 M H2SO3. (ii) Calculate the pH of a solution of 0.100M NazSO.. (iii) Calculate the pH of a solution resulting when equal volumes of the solutions described in parts (i) and (ii) are mixed.Calculate the pH of each of the following solutions. (a) 0.109 M HONH, (Ko = 1.1 x 10-3) 4.0 9.34 X (b) 0.109 M HONH3CI 4.0 2.64 (c) pure H₂O 7.00 X (d) a mixture containing 0.109 M HONH₂ and 0.109 M HONH₂CI 4.0 6.20 XAt 50 °C, the ion-product constant for H2O has the valueKw = 5.48 x 10-14. (a) What is the pH of pure water at50 °C? (b) Based on the change in Kw with temperature,predict whether ΔH is positive, negative, or zero for theautoionization reaction of water:2 H2O(l) ⇌ H3O+(aq) + OH-(aq)