How many grams of NaOH (MW=40.0 g/mole) do you need to add to 50.0 ml of a 0.2 M weak acid HA (Ka=4x10-6) to get a pH of 6.2?

Q: How many grams of sodium hydroxide would be required to prepare a 751.0 mL solution of sodium…

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Q: What is the pH of an acetic acid solution (HC2H3O2) with concentration 0f 0.100 M. Ka=1.75 x 10-5 A.…

A: An ICE table is constructed to determine the equilibrium concentration of H3O+ as follows,

Q: Calculate the pH of a 0.0488 M aqueous solution of acetylsalicylic acid (aspirin) (HC9H7O4, Ka =…

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Q: aqueous solutions will have a pH of 2.00 at 25 °C? (Kw = 1.01 × 10–14) 0.020 M HNO3

A: As we know,  Acidic solution has pH less than 7. Basic solution has pH greater than 7 . pH =…

Q: Determine the pH of 5.416 x 10-8 M of HCl. (use the systematic treatment) Determine the pH of 7.814…

A: 1)  Concentration of  HCl solution = [HCl] = 5.416 x 10-8 M pH of the solution = ? Note: HCl is a…

Q: Lactic acid, HC3H5O3, is found in sour milk. What is the pH of 0.30 Mlactic acid? (Ka = 1.4 ××…

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Q: What is the Kw of pure water at 50.0 degrees Celsius, if the pH is 6.630

A: A numerical problem based on equilibrium concept that is to be accomplished.

Q: The Ka value for acetic acid, CH3COOH(aq), is 1.8×10 −5. Calculate the pH of a 1.40M acetic acid…

A: Acetic acid dissociate in aqueous solution as: CH3COOH→CH3COO-+H+

Q: 7. If a neutral solution of a water , with pH= 7.00, is cooled to 10oC, the pH rises to 7.27. Which…

A: Water can react with itself in a weak acid-base equilibrium to create hydronium ion and hydroxide…

Q: 4.0 g of baking soda (NaHCO3 , 84.02 g/mol) is fully dissolved in 100.0 mL water.  What is its pH?…

A: NaHCO3 is an amphiprotic species. That is, it can act as acid as well as a base.  The pH of such…

Q: Determine the pH of 80 mL of a 0.30 M solution of acetic acid when 0, 40 mL, 80 mL and 100 mL  of…

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Q: 3. Create a table showing the [H3O+] that corresponds to each of the 5 pH readings.

A: 3. pH is defined as the negative logarithm of hydronium ion H3O+ concentration of base ten .The…

Q: Ammonia has a pKb=4.75. Work out how much ammonia is in the form of NH4+ in a 0.01 Molar solution at…

A: Ammonia in water exists as: NH3+H2O↔NH4OH→NH4++OH-

Q: What is the pH of 0.1000 M Na₂HPO4? (K₁2=6.2x10-8, K3=4.8x10-13) What is the pH of 0.1000 M Na3PO4?…

A: The solutions considered are 0.1000 M Na2HPO4 and 0.1000 M Na3PO4. The question requires to…

Q: How many mL of 0.360 M H2SO4 is needed to neutralize 25.00 mL of 0.233 N Ba(OH)2?

A: The given data contains, Concentration of H2SO4 =0.360 MVolume of H2SO4=-Concentration of Ba(OH)2…

Q: What is the pH of a solution with [H3O+] =  1 x 10-9 M? Group of answer choices 1 x 10-5 9 5 -5

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Q: Complete the following statements about the below solutions at 25 °C? 1. The pOH of 9.95 x 105 M KOH…

A: at 25°C ;  pH + pOH = 14.0  pOH = -log[OH-]

Q: The concentration of H+ ions in milk is 6.16 x 10-7 mol/L . What is the pH of milk? Express your…

A: The pH of any solution is given by the following formula…

Q: at 95 ℃ water has an autoionization constant (Kw) of 4.518 X 10-13. Determine the ph of pure water…

A: Given :- Kw at 95°C = 4.518 × 10-13  To determine :- pH of pure water at 95°C

Q: 13. What is the pH of a solution with [H3O+] = 3.0 × 10-3 M?   Group of answer choices 3.0 2.52…

A: pH :-  The negative logarithm to the base 10 of hydronium ion concentration , [H3O+] expressed in…

Q: 2. Do you expect the equivalence point to be below a pH of 7, equal to a pH of 7, or above a pH of…

A: Equivalence point is that stage of titration at which amount of titrant added is enough to…

Q: A generic weak acid was prepared and has a concentration of 0.471 M. Its Kb value is 4.91x10-10.…

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Q: Calculate the pH of a 2.80×10-1 M aqueous solution of sodium acetate (NaCH3CO2). (For acetic acid,…

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Q: If you start with 50 mM acetic acid, 20 mM acetate (pKa = 4.76) solution, how much of a 0.20 M…

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Q: A solution with a pH of 7 has a [OH1-] of Group of answer choices 1 x 10-7 M 0 M 1 x 10-14 M 7 M

A: Given is, pH= 7

Q: a solution is made from 0.23 M CH3NH2 (a weak base) and 0.24 M CH3NH3Cl. what is the pH of the…

A: The pH of this buffer solution can be calculated by using Handersson-Hesselbalch equation-

Q: is the pH of a 1.000 L solution of 0.100 M HA after the addition of 1.000 L of 0.075 M NaOH? The K₂…

A: Volume of HA=1L Molarity of HA=0.1M Volume of NaOH=1L Molarity of NaOH=0.075M  K2 of HA=6.78×10^-8…

Q: Calculate the pH of each of the following solutions at 25°C. 0.135 M HONH2 (Kb = 1.1 x 10-8) 0.135…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: The concentration of H+ ions in milk is 6.6 x 10-7 mol/L. What is the pH of milk? Express your…

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Q: A 0.250 M solution of a weak base has a pH of 9.91. Calculate the Kb of this base. Kb = ______ x…

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Q: Calculate the pH of a 0.094 M solution of formic acid, H2CO2. The Ka of formic acid 4 x 10-4 Submit…

A: In case of weak acids , the H+ ion concentration is given by the following formula  [H+] = (Ka×C)1/2…

Q: Calculate the pH when 1.03 g of NaClO (FW = 74.44 g/mol) is added to 44.4 mL of 0.50 M HClO. Ignore…

A: Answer: In this question we have to calculate the pH of the buffer made of HClO and NaClO.

Q: 1. What is the pH of 0.25L of chicken soup? How about 0.5L? Is it acidic or basic? 2. Does the pH…

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Q: Which of the following has the lowest pH?   3.9x10-3 M HPO42- (Ka3=4.2x10-13)   0.00010 M H3BO3…

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Q: A. Calculate [OH−] for 1.1×10−3 M Sr(OH)2 Express your answer using two significant figures.

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Acetic acid is a weak acid with Ka = 1.8 x 10 -5 and ionizes into HC2H3O2 -------H + + C2H3O2 - What…

A: pH is negative logarithm of hydrogen ions

Q: What is the pH of a 0.712 M weak acid solution that has a Ka = 4.5 x 10-9?

A: Weak acids dissociate partially. So we have to calculate degree of dissociation first and then pH.

Q: Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50 Group of answer…

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Q: b. The Ka of salicylic acid is The [H+] in the 0.1 M salicylic acid solution is M. The pH of a 0.1 M…

A: In this question we are dealing with two weak acids i.e aspirin and salicylic acid whose pka values…

Q: the pH of a solution of 15 g NH4Cl and 15 g of NH3 in a 850mL solution? The Kb for NH3 is 1.8 x 10-5

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Q: Calculate the pH, [OH-], and pOH of a.) Black coffee, 5.0 x 10 -5 M H+ b.) 0.125 M HC2H3O2, Ka =…

A: Calculate pH, [OH-] & pOH of the given solutions--

Q: What is the pH (to two decimal places) of a 50.0 mL 0.15 M NH3 aqueous solution (at 25 °C) after…

A: Given data,Molarity of NH3=0.15MVolume of NH3=50mL=0.050LMolarity of HCl=0.20 MVolume of…

Q: c. 10-8 M HNO3 solution? d. a solution containing 12.2 g KOH dissolved in 800 ml solution. e. a…

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Q: A 0.10 M sample of a weak acid has a Ka of 4.0 x 10 −5. What is the pH of the weak acid? Between 3…

A: Let HA be the weak acid. It ionizes in the solution as follows:                               HA…

Q: Write the acid concentration or the pH for each of the following instances: A.) a 0.5 M solution…

A: A.) a 0.5 M solution H2SO­4:

Q: Find the pH of a 0.4M aqueous hydrocyanic acid solution. For HCN, Ka=4.9 x 10^-10     4.85…

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Q: For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than…

A: The approx pH of the mixture of acid and base would be decided by the strength of acid and base .

Q: Hydrofluoric acid (HF) has a Ka value of 7.2 x 10^-4. What is the pH to 2 decimal places when 13.75…

A: Given : Ka=7.2×10-4 Volume of KOH=13.75 ml Molarity of KOH=1.074 M Volume of HF=27.5 ml…

Q: What is the pH of a 0.0100 M solution of acetic acid? Ka=1.8x10-5

A: Dissociation of acetic acid can be written as; CH3COOH →   CH3COO- + H+ Given that concentration of…

Q: What is the pH of a solution in which 21.65 mL of 0.28 M HNO3 is added to 9.95 mL of 0.067 M…

A: HNO3 is strong acid Ba(OH)2 is strong base.

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.