Q: What is the pH of a 3.50 M solution of NH4CI (Ká of NH3= 1.8 x 105)?
A:
Q: A solution is prepared at 25 °C that is initially 0.17M in acetic acid (HCH,Co,), a weak acid with…
A:
Q: Calculate the pH of a 0.381 M NH, solution. NH, has a Kp = 1.8 x 10-.
A: pH: The negative logarithm of H+ ion concentration is known as pH. Ammonia in water behaves as a…
Q: Would you expect Fe2+ to be the stronger Lewis acid? Explain.
A: A Lewis acid is a substance that accepts a pair of electrons. A Lewis base is a substance that…
Q: 2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH);SOu. a) What is the pH of…
A: “Since you have asked multiple questions, we will solve the first question [Q2] for you. If you want…
Q: What is the pH of a 0.0500 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?
A: HONH3Cl is a salt and in solution it gets dissociated as HONH3Cl → HONH3+ + Cl- The hydrolysis…
Q: What is the pH of a 0.0730 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?
A: Given :- concentration of methylamine solution = 0.0730 M Kb for methylamine = 4.4 × 10-4 To…
Q: What is the pH of a 0.0250 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?
A: pH can be calculated as follows
Q: A solution is prepared that is initially 0.0010 M NaOH and 0.10 M NH3. What is the pH of this…
A: [NaOH] =0.001 M [NH3] = 0.10M
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 of a solution containing 0.1M NH,OH and 0.01M NH.CI, K = 1.76 x 10$. %3D
A: Given, [NH4OH] = 0.1 M [NH4Cl] = 0.01 M Kb = 1.76 × 10-5
Q: | Calculate the pH of a solution which is 0.345 M NHẠCI. (Kô of NH3 = 1.80 x 105)
A: Introduction: An acid is defined as substance which can donate protons and base which can accept…
Q: Find the pH of a 0.20 M aqueous solution of benzoic acid, for which Ka = 6.33 x 10-5
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Q: What is the pH of a 0.0650 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?
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Q: What is the pH of (i) 1.0 X 103 M HBr and (ii) 1.0 X 102 M KOH?
A: We know that, pH and pOH can be expressed as the negative logarithm of hydrogen ion and hydroxide…
Q: What is the pH of a 0.620 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10 4)?
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Q: What is the pH of a 0.820 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?
A: The pH of the solution is equal to the negative logarithm of hydronium ion while pOH of the solution…
Q: Fill in the left side of this equilibrium constant equation for the reaction of carbonic acid…
A: in this question given ka ka= Acid dissociation constant, acid dissociation constant is used to…
Q: Calculate the pH of the solution that contains 0.145 M NH3 and 0.192 M NH4Cl. The Ka of NH4+ is…
A: The solution will be the buffer solution if the weak acid and its corresponding conjugate base are…
Q: What is the pH of a 0.050 M triethylamine, (C2HS)3N, solution? Kb for triethylamine is 5.3 x 10-4
A: We should know that the amine us a basic Compound that will dissociate in solution to give basic…
Q: What is the pH of a mixture of 0.042 M NaH2PO4 and 0.058 M Na2HPO4?
A: Given : Concentration of NaH2PO4 = 0.042 M Concentration of Na2HPO4 = 0.058 M
Q: Determine the K, of a weak base if a 0.28 M solution of the base has a pH of 10.14 at 25°C. K x 10
A: Given: Concentration of weak base (Assuming B) = 0.28 M And the pH of the solution = 10.14
Q: 16. The Ka of Hydrocyanic acid is 4.9 X 10-10 Consider a 0.050 M solution of its salt potassium…
A: To Find: To find the pH value of the salt solution.
Q: A solution is prepared at 25 °C that is initially 0.31M in propanoic acid (HC,H,CO,), a weak acid…
A: Given, Concentration of propanoic acid (HC2H5CO2) = [HC2H5CO2] = 0.31 M Concentration of potassium…
Q: What the pH of 0.10 M solution of methylamine (Kb for CH3NH2 is 4.4 x 10*)?
A: A numerical problem based on pH of the weak base, which is to be accomplished.
Q: A solution is made with 3.825 g NH,CI, dissolved in enough water to make 625 mL of solution. If the…
A: First, we calculate the concentration of the solution. After that, we calculate the [OH-] with the…
Q: What is the pH of 0.0100 M potassium phthalate (K2P)?
A: The acid ionization constant, Ka of potassium hydrogen phthalate (KHP) is 3.91×10-6. The dipotassium…
Q: Calculate the pH of a 0.633 M NH, solution. NH, has a Kp 1.8 x 10–5.
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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 0.690 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?
A: HNO2 ⇌ H+ + NO2- Ka = 4.5x10-4 = [H+][NO2-]/[HNO2] 4.5x10-4 = (x)(x)/0.690 - x if we assume x is…
Q: 1. Calculate pH and concentrations of the ions for ammonia aqueous solution with concentration 0.010…
A: Given that : The concentration of ammonia = 0.010 M The pKb of ammonia is 4.76. We have to calculate…
Q: Determine the pH at 25C of a solution prepared by dissolving 0.35 mole of ammonium chloride in 1. L…
A: Concentration of ammonia Volume of ammonia solution Number of moles of ammonium chloride added =…
Q: What is the pH of a 0.0930 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?
A:
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: 8. What is the pH of a 0.20 M solution of sodium acetate? The K, for acetic acid is 1.8 x 10-5 ?
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Q: What is the pH of the following solution? Hydrogen sulphide is a weak acid and has a pka of 8.9 x…
A: Please be noted that the value given for H2S is Ka not pKa. Therefore, pKa(H2S)=8.9×10-8.
Q: 0.3728, 0.9319, 1.4910 and 1.8638 g aliquots of KCI were dissolved in 4 separate 250 ml samples of…
A: KCl is a salt of strong acid and strong base. As a result, it doesn't undergo hydrolysis when…
Q: What is the pH of a 0.600 M solution of HSO, (Ka = 6.6 × 10°)? (Please show your answers with 3 sig…
A: pH of solution is equal to the negative logarithm of hydronium ion concentration. pH=-log(H3O+) Ka…
Q: Is it possible for an aqueous solution to have a pH of 0 or even less than 0? Explain your answer…
A: pH : 1. pH of an aqueous solution depends on the concentration of H+ ions. pH = -log [H+] 2.…
Q: what is the ph of 0.0349 M anilinium hydrochloride (C6H5NH3CI) solution in water, given that K for…
A:
Q: Determine the pH of a solution created by dissolving 0.255 g of magnesium hydroxide (MW = 58.3…
A: Mass of magnesium hydroxide=0.255 g MW= 58.3g/mol Volume=325 mL pH of solution=?
Q: The pH for a solution with an [OH] of 1.0 x 10^-6 is?
A: We have Concentration of OH- as 10-6 , we have to predict the pH of Solution.
Q: A 0.495 M solution of a weak base has a pH of 11.00. What is the base hydrolysis constant, Kp, for…
A:
Q: 6. Calculate pH for the 0.05 M Ca(OH)2 and 0.01M HCl and explain the natures of the solutions after…
A: Ca(OH)2 pH-13 HCl pH- 2
Q: A solution is prepared at 25 °C that is initially 0.30 M in benzoic acid (HC,H,Co,), a weak acid…
A: Step 1: The given solution is a buffer of weak acid and its conjugate base. So, the Handerson…
Q: What is the pH of a 0.680 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 104)?
A: Given, The pKa value of HNO2=4.5×10-4 Molarity of Ca(NO2)2= 0.680M.
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- 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.In the laboratory, a general chemistry student measured the pH of a 0.433 M aqueous solution of phenol (a weak acid), CoH5OH to be 5.167. Use the information she obtained to determine the K, for this acid. K₂(experiment) =1) Calculate the pH of a solution prepared by dissolving 1.90 g of sodium acetate, CH,COONA, in 64.0 mL of 0.15 Macetic acid, CH;COOH(ag). Assume the volume change upon dissolving the sodium acetate is negligible. K, of CHCOOH is 1.75 x 105. Calculate the amount of heat released or absorbed by the following substance: 90.23g of iron, AT= 86°C Calculate the amount of heat released or absorbed by the following substance: 7.45g of silicon, final temperature = -10°C, initial temperature = 25°C
- In the laboratory, a general chemistry student measured the pH of a 0.597 M aqueous solution of phenol (a weak acid), C6H;OH to be 5.098. Use the information she obtained to determine the K, for this acid. K(experiment) =650.0 mL of HBr gas at 21.0 °C and 1025 mm Hg is absorbed completely into a solution that was created by mixing 7.147 g of Na2CO3 and 250.0 g of water. (a) What is the pH of the solution? (b) What is the freezing point of the solution?3.134 grams of potassium sorbate (KCH3(CH,)4CO2 ) is fully dissolved in 100.00 mL of water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.240 M HNO, is added dropwise to this solution from a burette. Given: K, (sorbic acid) = 1.7 x 10-5. Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above.
- Which of the following pairs of solution would you use to prepare a buffer with pH = 7.45? (A) Acetic acid + sodium acetate; (CH3CO2H has Ka = 1.8 x 10–5) (B) Sodium dihydrogen phosphate + sodium hydrogen phosphate; (H2PO4– has Ka = 6.2 x 10–8) (C) Ammonium chloride + ammonia; (NH3 has Kb = 1.8 x 10–5) (D) Sodium hydrogen carbonate + sodium carbonate; (HCO3– has Ka = 5.6 x 10–11)7) An aqueous solution containing 25.0 mg of a hormone in 150.0 mL of solution with an osmotic pressure at 25 °C of 9.00 mmHg. What is the molecular weight of the hormone? 8) (a) What is the pH of a solution in which 45 mL of 0.10 M sodium hydroxide is added to 25mL of 0.15M hydrochloric acid? (b) A brand of carbonated beverage has a pH of 3.50. Calculate [H*]=?A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.
- 33. Consider a buffer solution that contains 0.45 M HCOOH and 0.55 M NaHCOO. Note that the Ka for formic acid (HCOOH) is 1.8 x 104. (a) Calculate the pH of this buffer solution. pH = (b) Write the net ionic chemical equation that occurs when potassium hydroxide (KOH) (MW of KOH = 56.1 g/mol) is added to the buffer. (c) If 0.260 g of solid KOH is added to 250. mL of this buffer solution, what is the resulting pH of the solution? New pH =You prepared 500 mL buffer solution that contains 0.50 moles monoprotic weak acid (HA) and 0.30 moles conjugate base (NaA). The solution has a pH of 4.20. (a) What is the Kp of the conjugate base, NaA? (b) What is the pH of the buffer solution after adding 400 mL of 0.30 M H,SO4? pH = pKa – log(THA), [A*]Your answer is partially correct. Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer solution containing 46 g of NH4CI dissolved in 1.00 L of 0.920 M NH3? pH = 9.24 (b) How many moles of acid are required to change the pH of this solution by 0.07 pH units? i 5.5E-2 mol (c) Suppose 4.8 mL of 11.8 M HCI solution is added to 146 mL of the solution of Part (a). Calculate the new pH. pH = i 9.08 eTextbook and Media Save for Later Attempts: 1 of 3 used Submit Answer