Q: Calculate the pH of a 0.40 M solution of(C2H5)2NH (Kb=1.3x10^-3)
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Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.200 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)
A: By using Henderson Hasselbalch equation the pH of the buffer solution is determined by using the…
Q: What is the pH of a 0.150 M solution of aniline (CeH;NH2, Kb = 4.3 × 10-1º)?
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Q: action. Ighore inorganic byproducts and C2. 1. KMNO4, OH- (warm) 2. H3O* Select to Draw
A: When alkene is treated with alkaline KMnO4 followed by acidification under heating condition then…
Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.170 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)
A: pH of a solution is defined as the negative logarithm of H3O+ ion concentration. Here the given…
Q: Calculate the Ka of a 0.400 M acid solution with [H30*]= 1.4x 10 4M O 1.40 x 106 O 1.40 x 10 5 O…
A: Equilibrium constant is defined as products concentrations divided by reactant concentrations to the…
Q: Fill in the left side of this equilibrium constant equation for the reaction of benzoic acid…
A: The Equilibrium constant for a reaction A + B ⇔ C + D Can be written as K = [C][D][A][B],…
Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.110 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)
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Q: Calculate the pH of a solution containing 0.03 M NaH2VO4, and 0.05 M Na2HVO4 (Ka1- 1.11.10-2, Ka2 =…
A: Please be noted that the formula of the compound is NaHVO4- but not Na2HVO4. pH=- log H+ For a…
Q: What is the pOH of a solution that has a H3O+ concentration equal to 8.23 x 10-5 M at 25°C?
A: The sum of pH and pOH is equal to 14. So from pOH value also we can know that the solution is…
Q: What will be the pH of a solution containing 0.200 M NaH2PO4 and 0.200 M Na2HPO4? Ka(NaH2PO4) = 6.2…
A: Given, Molar concentration of weak acid, NaH2PO4 or H2PO4- = [H2PO4-] = 0.200 M Molar concentration…
Q: Calculate the pH of a 0.350M aqueous solution of NH3 , The Kb of NH3 is 1.77 x 10-5
A: Given: The concentration of aqueous NH3=0.350M
Q: What is the pH of a 0.03 M solution of sodium benzoate (C6H5COONa)? Ka = 6.6 *10-5.
A: It is given that 0.03 M sodium benzoate (C6H5COONa) is present, and the equation is written as…
Q: Find the pH of 0.15 M HClO and 0.25 M NaClO. Ka of acid at 25 C is 3.98 x 10^-8
A: Given data The concentration of HClO, [HClO] = 0.15 M The concentration of NaClO, [NaClO] = 0.25 M…
Q: What is the pOH of 0.92 M RBCIO4?
A: Given : Concentration of RbClO4 = 0.92 M
Q: could you please answer and show working to the following questions 1. What is the pH of a…
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Q: New August 9, 2020. Which solvent could differentiate between the strength of NAOH and KOH is Select…
A: Both NaOH and KOH are strong bases so to differentiate between their strength we need an acid.
Q: Claculate pH for a strong base solution: 10 mL of 1.8 x 10-2 M Ca(OH)2 diluted to 520.0 mL.
A: The solution is diluted to 520.0mL. The molarity will change. The new molarity can be calculated…
Q: What would be the pH of a 0.100 M acetic acid solution (Ka = 1.74 x 10-5)?
A: Given : Concentration of acetic acid i.e CH3COOH = 0.100 M And Ka of acetic acid = 1.74 X 10-5…
Q: Calculate the [H+] in 8.8 x 10^-4 MCa(OH)2 solution
A: Ca(OH)2 --> Ca2+ + 2OH- Concentration of Ca(OH)2 = 8.8×10-4 , so ,[OH-] = 2 ×8.8×10-4 =…
Q: Calculate the pH of a 0.299 M NH, solution. NH, has a Kp = 1.8 × 10-5. pH =
A: pH =11.366
Q: Use the information provided to determine the Ksp of the salt. A saturated iron(II) hydroxide…
A: Equilibrium reaction of iron(II)hydroxide: Fe(OH)2(aq) ⇌ Fe2+(aq) + 2OH-(aq) pH + pOH =1410.62 +…
Q: Calculate the pH and pOH of 0.30 M HNO3 solution. Kw= 1.0 x 10-14
A: Given data: Concentration of HNO3 solution = 0.30 M, Kw = 1.0×10-14. Nitric acid (HNO3) is the…
Q: Calculate the pH of 0.1 M from sodium acetate CH3CO2Na and hydrolysis percent ? if you know Ka =…
A: Reaction of sodium acetate in water can be written as, CH3COONa + H2O →CH3COOH +Na+ + OH-
Q: Calculate the Ka of a 0.390 M acid solution with [H3O+]= 4.52 x 10-5M
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Q: What is [H⁺] in a 0.310 M solution of acrylic acid, CH₂CHCOOH (Ka = 3.16 × 10⁻⁵)?
A: Molarity of acrylic acid = 0.310 M Ka = 3.16 × 10-5 [H+] = ?
Q: What is the pH of a 0.32 M solution of a weak acid, HCNO if Ka for HCNO is 2.0 x 10-4? (SHOW…
A: a) Given that, Molarity of HCNO solution = 0.32 M Ka value of HCNO acid = 2.0×10-4 HCNO is a weak…
Q: Calculate the pH of 3.5M citric acid solution at 25⁰C when the Ka is 7.1 x 10-4.
A: Give information: Concentration of solution = 3.5 M Ka is 7.1 x 10-4
Q: 6. What is the pH of 0.5 M nitrous acid (HNO2) ( Ka = 4.5 x 10-4) %3D www
A: Find the pH of HNO2 having 0.5 molarity Given ka = 4.5 x 10-4
Q: Calculate the pH of a 0.654 M solution of an acid with Ka = 2.33 x 10-5.
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Q: 0.1 M NH4CI solution, using the given pH data, calculate value of (Ka or Kb) 1.0 x 10-9 O 1.0 x 10-6…
A: Since NH4Cl is a salt of weak base and strong acid so we can use hydrolysis formula for this salt
Q: what would the pH of the solution be?
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Q: Determine the pH of a 0.0525M Fe(NO3)3 solution. Ka of Fe3+ = 6.3x10-3
A: Reaction of ferric nitrate in water is given below Fe3+ is formed from Fe(NO3)3.
Q: What is the pH of a solution of 0.300 M HNO2 containing 0.120 M NaNO2? (Ka of HNO2 is 4.5 × 10¬4)
A: The given data contains, Concentration of weak acid =0.300M Concentration of conjugate base =0.120M…
Q: What are the concentrations of H3O+ and OH− in oranges that have a pH of 3.97?
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Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.150 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)
A: In this question, we will calculate the pH of this solution ( this is a buffer solution ). For…
Q: What is the pH of a solution that is 0.05M in ethylamine and 0.08M in its chloride salt (pKa=10.8)
A: pH of a solution =? [ C2H5NH2 ] = 0.05 M [ C2H5NH3+ ] = 0.08 M Acid dissociation constant :…
Q: Nahso3 titr. In neutral describe how the color goes from Mn04- to MnO2 In basic w NaOH describe…
A: Answer-1 In neutral medium, SO32- ion of NaHSO3 is oxidized by MnO4- ion into sulfate ion and MnO4-…
Q: What is the pH of a 0.64 M solution of NH3 (Kb = 1.2 × 10-5)?
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Q: Calculate [H+], PH and POH respectively of CH3COOH solution has concentration 1.0 x 10-3 M and the…
A: Here i have calculated all the things
Q: Determine [H30*] of a 0.250 M solution of formic acid (Ka 1.8 x 10-4).
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Q: What is the pH of a solution of 0.400 M CH;NH2 containing 0.140 M CH;NH31? (Kb of CH;NH2 is 4.4 ×…
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Q: Calculate the pH of 0.0154 M NaN3. (Ka of HN3 = 1.9 x 10-5)
A: NaN3 is a salt of weak acid (HN3) and strong base (NaOH). We know, the pH of salt, which is formed…
Q: What is the pH of a solution that has a [H3O+] of 7.2 x 10-3? please show work to help me better…
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Q: The acid ionization constant for Sc(H2O)63+ (aq) is 5.0×10-5 . Calculate the pH of a 0.0043 M…
A: Given , acid ionisation constant , Ka= 5.0×10-5 concentration of the Sc(NO3)3= 0.0043 M
Q: Calculate eq. concentrations when for 0.55 M HAc solution where ka(25C)=1.8x10^-5 with an ICE table.…
A: Look out this reaction as: HAc: concentration of acetic acid. H+: concentration of proton. Ac-:…
Q: Calculate the pH of a solution that is 0.553 M nitrous acid (HNO2) and 0.663 M of potassium nitrite…
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Q: What is the pOH of a solution with [OH-] = 6.22 x 10^-5 %3D
A: The formula for pOH is as follows: pOH=-log([OH-])…
Q: What is [H*] in a 0.270 M solution of acrylic acid, CH2CHCOOH (Ka = 3.16 x 10-5)?
A: Using the equilibrium concept We can calculate the H+ concentration
Calculate the pH and pOH, respectively, of an ammonia based cleaner with an [OH-] of 3.81 x 10-2 M at 25 0C
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- 2. Calculate pH and pOH for each of the following solutions and determine whether thesolution is acidic, basic or neutral:(i) [H3O+] = 4.1 x 10-10 M (ii) [OH–] = 7.6 x 10-3 M(iii) [OH–] = 6.9 x 10-4 M (iv) [H3O+] = 3.5 x 10-6 M10. How many moles of CH;COONA (sodium acetate) must be added to 2.0 L of 0.10 M CH;COOH (acetic acid) to give a solution that has a pH equal to 5.00? Ignore the volume change due to the addition of CH;COONA (sodium acetate). The Ka of CH;COOH = 1.8 x 105. (Note – the Na at the end of the molecule is the same as the Na at the beginning - it just drops off).3a) Write the hydrolysis reaction of a 0.050M solution of acetic acid. Clearly identify the acid, base, conjugate acid, and conjugate base in the reaction. b) is this acid a strong acid or weak acid? Why? c) calculate the [H3O+] for this reaction (hint: Use an ICEq box) d) calculate the pH of a 0.050M solution of this acid
- The acid dissociation constants for sulfurous acid are: Ka1 3D 1.2 х 10-2 and Ka2 - 6.6 х 10-8 (a) Calculate the pH of a solution of 0.10 M H2SO3. (b) Calculate the pH of a solution of 0.10 M Na2SO3. (c) Calculate the pH of the solution resulting when equal volumes of the solutions described in parts (a) and (b) are mixed.8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? 9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)Calculate 3OH-4 and pH for each of the following strong base solutions: (a) 0.182 M KOH, (b) 3.165 g of KOH in 500.0 mL of solution, (c) 10.0 mL of 0.0105 M Ca1OH22 diluted to 500.0 mL, (d) a solution formed by mixing 20.0 mL of 0.015 M Ba1OH22 with 40.0 mL of 8.2 * 10-3 M NaOH.
- 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 X2. Determine [H3O+] and [OH] concentrations (in M to two decimal places) for each: (a) Pure water at 10 °C (K = 0.293 x 10-14) W (b) An aqueous solution with a pH of 3.23 A: 5.41x108; 5.41×10-8 A: 5.89x104; 1.70×10-11Calculate the pH and the pOH of these solutions: (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH = pOH =
- 6. In a 0.050 M solution of HC1 at 25°C, (a) What is the H3O* concentration? (b) What is the OH concentration? 7. Write a balanced reaction for the dissociation of HOC1 in water. 8. Write the expression for the Ka of HOCI. -2- 9. (a) If 0.30 moles of HOCI are added to water to make a 1.0 L solution at 25°C, what would be the algebraic expressions for [HOC1] and [H3O*] at equilibrium? Note that you should use your answers to #7 and #8 for this. (b) What is the algebraic expression for [OH-] at equilibrium? Use part (a) and previous concepts to answer this. 10. The Ka for HOCI is 2.9 x 10-8 at 25°C. What is the concentration of H3O* and OH¯ at equilibrium? 215 >Please answer these questions on your Page 8 (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 7.7 x 10-¹2. What is the pH of a 0.011 M solution of A-(aq)? The temperature is 25°C. (b) For the reaction A(g) A(1), the equilibrium constant is 0.666 at 25.0°C and 0.111 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?5a) Write the hydrolysis reaction of nitric acid Clearly identify the acid, base, conjugate acid, and conjugate base in the reaction. b) is this acid a strong acid or weak acid? Why? c) calculate the [H3O+] for a 0.050M solution of this acid d) calculate the pH of a 0.050M solution of this acid
