50 mL of 0.02 M NaOH is added to 25 mL of 0.04 M HCl solution. The pH of the resulting solution will be?   A. 2 B. 1.7 C. 1 D. 7

Q: 1 A student dilutes a 0.25 M HCI solution to obtain a 0.025M solution. The student then measures the…

A: Concentration of the diluted HCl solution = 0.025 M Measured pH of the diluted HCl solution = 1.75…

Q: Calculate the pH of the following: (a) 500 ml of pure water (b) 15.0 mL of 2F hydrochloric acid…

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Q: You make 1.00 L of a buffered solution (pH=4.20) by mixing acetic acid and sodium acetate. You have…

A: The pKa is calculated as follows:

Q: When 0.20 mol of NaOH is added to 0.50 mol of weak acid HX, in a total volume of 1.00 L, the pH of…

A: This acid - base reaction between NaOH and weak acid HX form a buffer solution. So we will use…

Q: Calculate the pH of a 200 mL solution of pure water to which has been added 50 mL of 1 mM HCl.

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Q: A 0.667 M solution of a weak base has a pH of 10.80. What is the base hydrolysis constant, ?b, for…

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Q: Calculate the ph of the solution that is formed by diluting 55 Ml of 0.023 mole/L hydroxide acid to…

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Q: A sample of 1.25 L of HCl gas at 21 °C and 0.950 atm is bubbled through 0.500 L of 0.150 M NH3…

A: According to ideal gas law (for HCl moles calculation), PV = nRT where P = pressure = 0.950 atm V =…

Q: For 280.0 mL of pure water, calculate the initial pH and the final pH after adding 0.024 mol of NaOH

A: pure water : pH = 7.00 moles NaOH = 0.024 [OH-]= 0.024 mol/ 0.280 L=0.0857 M pOH = - log 0.0857=…

Q: b) To 1 L of the solution in part (a) are added 0.010 moles of solid Sodium Hydroxide (which…

A: This can be solved by finding the concentration of that base and acid. That can be solved by…

Q: For 550.0 mLmL of pure water, calculate the initial pH and the final pH after adding 0.020 molmol of…

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Q: The pH of a household ammonia solution is 11.75. Calculate the mass of ammonia needed in a 2.50 L…

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Q: A solution is prepared by diluting 20.0 mL of 0.0010 M HCl to a final volume of 2.00 liters. What…

A: Consider the given information is as follows; Volume of initial HCl solution V1= 20.0 mL = 0.02 L…

Q: Consider a HCl solution that has a pH of 4.70. a) Calculate the concentration of HCl.  b) Identify…

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Q: A 15 ml solution is 0.50 HCI. If 0.2 M NaoH is to added to this solution Calculate the pH of…

A: Given, Volume of HCl solution = 15 mL Concentration of HCl solution = 0.50  Concentration of NaOH…

Q: You are given three solutions: HCl (Solution A); NaOH (Solution B); pH = 8.76 solution (Solution S).…

A: Given: Three solutions: HCl (Solution A); NaOH (Solution B); pH = 8.76 solution (Solution S) As the…

Q: What mass of HCI should be used to make 175.0 ml of a solution with a pH of 2.80? The molar mass of…

A: Provided volume (V)=175ml Or, Provided volume (V)= 0.175litre Provided molar mass of HCl=36.46g/mol…

Q: For the treatment of his acidosis, Pran must drink a salt solution wi wanted to give Pran a 0.895 mM…

A: pH is known as the "potential of hydrogen". It is a scale used to specify the acidity or basicity of…

Q: • Part C How many milliliters of 14 M HCl must be added to 0.500 L of the original solution to…

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Q: 2. A 10.0 mL sample of 5.00M HCl is diluted until its final concentration is 0.215M. What is the…

A: Question 2 :- Initial volume of solution,V1 = 10mL Initial concentration of solution,M1 = 5.00M…

Q: The pH of an aqueous solution at 25°C was found to be 5.80. The pOH of this solution is .????? The…

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Q: Part A If 15.0 mL of glacial acetic acid (pure HC2H3O2; K₂ = 1.8 × 10−5) is diluted to 1.70 L with…

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Q: You make 1.00 L of a buffered solution (pH solutions of each component of the buffered solution.…

A: A buffer solution can be made using a weak acid and the conjugate base of the weak acid. For…

Q: A buffered solution is made by adding 80.0 g NH4 Cl to 1.00 L of a 0.90-M solution of NH3. Calculate…

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Q: Step by step please

A: The pH of the salt is calculated by using the equation,

Q: 48. A 0,25-g sample of lime (CaO) is dissolved in enough water to make 1500 mL of solution.…

A: As per our guidelines we can solve only first question please resubmit other questions as next…

Q: 2.500 g of an unknown achiral primary amine is dissolved in enough water to yield a 50.00 mL…

A: Given : mass of primary amine used = 2.500 g concentration of HCl used = 0.9250 M And volume of HCl…

Q: Calculate the pH when (a) 49.0 mL and (b) 51.0 mL of 0.100 M NaOH solution have been added to 50.0…

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Q: Calculate the pH of a 0.15 M NaF solution. b) Suppose you added 100.0 mL of 0.500 M HCl to 1.00 L…

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Q: Find the pH of a solution when 0.01 M HCI and 0.1 M NaOH are mixed in equal * volumes

A: The pH of a solution is defined as the negative logarithm of the concentration of the H+ present in…

Q: A chemist wants to make 20.00 L of a 0.25 M HCl solution. A) How many milliliters of a 11 M HCl…

A: A) Volume of 11M HCl required = 454.55 mL B) pH = 0.6021

Q: A 30.0 mL aliquot of a solution is 0.25 M HCl . If 0.1 M NaOH is to be added to this solution,…

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Q: a solution of NaOH is 0.2 M and has a density of 1.2 g / mol. a) What is the pH of this solution? b)…

A: Given : (a) [NaOH] = [OH-] = 0.2 M  pOH = -log[OH-] = -log 0.2 = 0.7  pH = 14 - 0.7 = 13.3  (b)  By…

Q: A general chemistry student mixes together a solution of HF with a solution of NaF. If the resulting…

A: Acidic buffer solution :- A mixture of weak acid and its salt with strong base is called acidic…

Q: . Calculate the resulting pH when 1.00 L of 1.00 M H,SO4 is added to a tank containing 1.00 × 107 L…

A: The dilution of base solution increases the volume of solution and also alter the molarity of…

Q: A 1.0m HCl solution has a volume of 60.0mL. Calculate pH of the solution that results from adding…

A: Since the moles = concentration X volume in L Hence moles of HCl = concentration of HCl X volume of…

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: An aqueous solution is prepared by dissolving 16.7 grams of Aluminum hydroxide in 645.0 mL solution.…

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Q: 21) a 10.0 mol sample of HCl is mixed with 5.0 mol sample of NH,OH in 150.0 milliliter solution,…

A: Following information given in the question - Moles of HCl in Solution = 10 moles Moles of NH4OH…

Q: Calculate the pH of the resulting solution when 70.00 mL of 1.000 M HCI is mixed with 65.00 mL of…

A: We have to calculate the pH of resulting solution.

Q: 50mL of a 2.0M HCl solution is diluted to 6,000mL with distilled water. what is the pH of the…

A: Using Equation of dilution and formula of pH , the pH of resulting solution can be calculated.

Q: 4. 4.00 g KOH was added to the less basic solution in number 3. What will be the resulting pH of the…

A: Given, Mass of NaOH = 5.00 g  Mass of Ba(OH)2 = 5.00 g  Gram molar mass of NaOH = 40 g/mol  Gram…

Q: B. Calculate the pH after 17.50 mL of NaOH is added to 35.00 mL of acetic acid using the…

A: pH of a solution is the negative logarithm of the concentration of H+ ions present in that solution.…

Q: in 2 liters of water dissolve 2.24 liters of HCl (g) measured under normal conditions. The resulting…

A: The volume of the HCl gas at NTP is = 2.24 liter The volume of the solution is = 2 liter The pH of…

Q: Suppose 90.00 ml of 0.200M HCI is added to an acetate buffer prepared by dissolving 0.100 mol of…

A: Volume of HCl = 90.00 mLConcentration of HCl = 0.200 MNumber of moles of acetic acid = 0.100…

Q: Calculate the pH of a formic acid solution that contains 1.44% formic acid by mass. (Assume a…

A: The density of solution is assumed as 1.01 g/ml. Assuming a volume of 1000 ml, the mass of solution…

Q: An aqueous solution contains 0.368 M hydrocyanic acid. Calculate the pH of the solution after the…

A: When a strong base is added to weak acid a buffer is formed. The pH of the buffer can be calculated…

Q: A solution is prepared using 15.0 ml of 1.0 M HCl and 20.0 ml of 0.50 M HNO3. The final volume of…

A: Given: (15 ml of 0.15 M HCl)  +  (20.0 ml of 0.50 M HNO3.) The total volume of the solution= 1.25 L…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.