A student mixes 300 mL of 0.100 M NaOH with 100 mL of 0.300 M H,SO4. The resulting solution has a pH of 14.000 0.000 13.800 O 7.000

Q: 1.00 L of a 0.0250 M solution of C9H7O4, adds 15.0 mL of aqueous sodium hydroxide . The pH of the…

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Q: Hydrocyanic acid, HCN, is a weak acid (Ka = 4.02*10-10). If I dissolve 0.882 g of HCN in enough…

A: Given information is as follows: The amount of HCN = 0.882 g The volume of water = 600 mL The value…

Q: A solution is prepared at 25 °C that is initially 0.057M in dimethylamine ((CH, NH) a weak base with…

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Q: If 8.5 grams of solid NaC2H3O2 (MW = 82.03 g/mol) are added to 100.0 mL of water, how many mL of 1.0…

A: Answer:- Henderson-Hasselbach equation :- This equation is used for the determination of pH or pOH…

Q: What is the pH of a solution

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Q: A chemist must prepare 450.0 mL of hydrochloric acid solution with a pH of 1.30 at 25 °C. He will do…

A: Volume of dil. HCl = 450.0 mLpH of dil. solution = 1.30molarity of conc. HCl = 9.0 M

Q: Suppose that 80.0 mL of an aqueous 0.200 M methylamine, CH3NH2(aq), is titrated with a 0.400 M…

A: The relation between pH and concentration of  acid and its conjugate base is calculated using the…

Q: 50.00 mL of 0.200 M sodium dihydrogen pyrophosphate (N22H2P207) solution is combined with 25.00 mL…

A: Buffer solution is prepared, when an strong base is added into weak acid solution then resulting…

Q: What would be the pH of a solution of hypobromous acid (HOBr) prepared by dissolving 9.7 grams of…

A: given:  mass of HOBr = 9.7 g molar mass of HOBr = 96.91 g/mo moles of HOBr = 9.796.91= 0.1 moles…

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00357 M HIO4 pH =  (b)…

A: Note: As per our guidelines, we are supposed to answer only three subparts. Please repost the other…

Q: A students mistakenly titrates 25.0 mL of a 0.20 M H2SO4 solution, with 62.0 mL of a 0.15 M NaOH…

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Q: A solution of sodium hypochlorite is made in 2.0 L of water.  The pH is determined to be 10.50.…

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Q: t is the pH of a 0. M solutI 350 M solution of NaOH is added? The K, of HA is 4.3 x 10-4.

A: We have to tell which option is correct from given choices of options by telling what is the pH of…

Q: A solution is prepared that is initially 0.22M in methylamine (CH, NH,), a weak base, and 0.31 M in…

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Q: students mistakenly titrates 25.0 mL of a 0.20 M H2SO4 solution, with 62.0 mL of a 0.15 M NaOH…

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Q: A quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 moles of sodium…

A: The ratio of the number of moles of a solute dissolved per litre of solution is called the…

Q: A chemist dissolves 369. mg of pure barium hydroxide in enough water to make up 60. mL of solution.…

A: Given: mass of Ba(OH)2=369 mg                                =0.369 gvolume of solution=60 mL To…

Q: A student is provided with a 1.0 M stock solution of hydrochloric acid (HCl) and asked to mix 5.00…

A: The dilution solution is prepared by reducing the concentration of solute in stock solution by…

Q: 1.0 M HCl solution has a volume of 20.0 mL. Determine the pH of the solution that results from…

A: The balanced chemical equation for the given reaction is,

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.000726 M HClO4 pH =…

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Q: A chemist must prepare 550.0 mL of nitric acid solution with a pH of 1.90 at 25 °C. He will do this…

A: Given that,  pH of 550 mL (V1) HNO3 solution at 25°C  = 1.90 Since, HNO3 is a strong acid and it…

Q: The pH of a white vinegar solution is 2.28. This vinegar is an aqueous solution of acetic acid with…

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Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00251 M HIO4 pH =  (b)…

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Q: Calculate the pH in the flask when 50mL of a 0.98 M HI solution have been added to 120. mL of a 0.77…

A: The question is based on the titrations.  we are titrating a strong acid with a strong base. we need…

Q: An analytic chemist is titrating 65.9 mL od 0.4200 M solution of piperidine (C6N10NH) with a 0.8800…

A: First calculate the number of moles for both given base and acid. Then use that moles to find out…

Q: A chemist must prepare 350.0 mL of hydrobromic acid solution with a pH of 1.80 at 25 °C. He will do…

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Q: Which one of the following values of [OH-] and pH is correct? A. 1.50 g of LiOH in 250. mL of…

A: 1.50 g of LiOH in 250. mL of solution has [OH-] = 0.251 M and pH = 0.601 Molar mass of LiOH =…

Q: A chemist dissolves 172. mg of pure barium hydroxide in enough water to make up 120. mL of solution.…

A: Molarity(M) of a solution is defined as the number of moles of solute present in the 1 liter of the…

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: when 100 ml of a .01 M Mg(OH)2 solution is mixed with 100 mL of a .01 M HCl solution, what is the pH…

A: Since both acids and base are strong  hence they will react to form water as shown below Mg(OH)2 + 2…

Q: What is the pH of a solution prepared by mixing 45.11 mL of 0.8314 M HCl and 42.03 mL of 0.7261 M…

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Q: The ?a value for acetic acid, CH3COOH(aq)CH3COOH(aq), is 1.8×10−51.8×10−5. Calculate the pH of a…

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Q: A chemist must prepare 400.0 mL of hydrochloric acid solution with a pH of 1.20 at 25 °C. He will do…

A: This problem can be treated under the topic of dilution. M1V1=M2V2 equation is used in such case.

Q: What is the pH of a solution that is prepared by adding 30.23 mL of 1.77 M NaOH to 0.646 L of 0.476…

A: THIS WILL FORM AN ACIDIC BUFFER AS THE AMOUNT OF WEAK ACID(HN02)WILL REMAIN IN EXCESS AFTER REACTION…

Q: A solution contains 0.302 M ammonium bromide and 0.201 M ammonia. The pH of this solution is

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Q: Equal volumes of 0.240 M weak base (Kb=4.0×10−9) and 0.240 M HCl are mixed. Calculate the pH of the…

A: The equal volumes of weak base and HCl means that all the weak base in the solution is converted to…

Q: The ?a value for acetic acid, CH3COOH(aq), is 1.8×10−5. Calculate the pH of a 2.40 M acetic acid…

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Q: A chemist must prepare 550.0 mL of hydrochloric acid solution with a pH of 1.10 at 25 °C. He will do…

A: We have to predict the volume of stock solution.

Q: Suppose that 80.0 mL of an aqueous 0.200 M methylamine, CH3NH2(aq), is titrated with a 0.400 M…

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Q: Calculate the pH of a solution that is 3.67×10−53.67×10-5 M NH3 and 2.41×10−52.41×10-5 M NH4Cl.…

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Q: A solution was prepared by 0.250 moles of ammonium chloride to 500.0 mL of 0.35 M ammonia. Given the…

A: For NH3 , pKb = -log Kb = -log ( 1.86 x 10-5 ) = 5 - log 1.86 = 5 - 0.27 = 4.73 Concentration of…

Q: The ka of an unknown acid, HYO₂,  is determined to be 5 x 10⁻² empirically. What is the pH of a 0.1…

A: The objective of this question is to calculate the pH of a 0.1 M solution of an unknown acid HYO2,…

Q: A solution contains 0.395 M ammonium chloride and 0.246 M ammonia. The pH of this solution is  1b.…

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.