alculate the pH of a titration solution formed when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of 0.100 M CH3COOH (Ka = 1.8×10-5).

Q: What is the [OH¯] of a solution after the titration of 25.00 mL of a 0.0250 M HCl solution with…

A: Given data,Molarity of HCl=0.0250MVolume of HCl=25.0mLMolarity of NaOH=0.05MVolume of NaOH=25.05mL

Q: 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of…

A:

Q: ) If 5.0 mL of 0.100 M NaOH is added to 100.0 mL of a 0.0500M phosphate buffer solution at pH 7.2,…

A: A solution which resists the change in pH when a small amount of acid or base is added to it,  is…

Q: Vhat is the pH of a solution containing 0.2 M citric acid (pKa = 5.4) and 0.1 M sodium citrate?

A: Introduction: Since having sodium citrate that is a buffer solution so we can use the…

Q: A buffer solution is 0.478 M in H3PO4  and 0.362 M in NaH2PO4 . If Ka1 for H3PO4  is 7.5 x 10^-3 ,…

A: According to the Henderson Hasselbalch equation is given by, Ph = Pka + log ([salt] / [acid] ) The…

Q: If 31.4 mL of a 0.75 M NaOH solution is added to a 47.1 mL sample of a 0.75 M weak acid, HA, what is…

A: Molarity of NaOH, M=0.75 M Volume of NaOH, V=31.4 mL Millimoles of NaOH=M x V (in mL)= 0.75 x 31.4…

Q: you mix 100. mL of 0.11 M HCl with 50.0 mL of 0.22 M NH3, what is the pH of the resulting solution?…

A: Volume of HCl=100.0mL Concentration of HCl=0.11M Volume of NH3=50.0mL Concentration of NH3=0.22M For…

Q: 6.5 g of sodium acetate was dissolved in 100 mL of water to give a final volume of 106 mL. If the Ka…

A: Sodium acetate dissociates in water into sodium and acetate ions. Sodium ions react very little with…

Q: What is the pH of the resulting solution if 30.00 mL of 0.10 M acetic acid is added to 10.00 mL of…

A:

Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: 2. Calculate the [H*] and pH in saturated solution of Ba(OH)2 , which contains 3.90 g of Ba(OH)2 per…

A: The dissociation of Ba(OH)2 : Ba(OH)2 ----> Ba2+ + 2OH-   Mass of Ba(OH)2 = 3.90 g  Volume of…

Q: What is the final pH when 0.032 mol of NaOH is added to 0.422 L of a solution containing 0.428M…

A: pH = pKa + log[C3H5O2-]/[HC3H5O2] Number of mol = Molarity x Volume (L)

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: 5. Calculate the pH of a buffer system containing 1.0 M CH,COOH and 1.0 M CH,COON..

A: 5. Given information,      1.0 M CH3COOH and 1.0 M CH3COONa

Q: If the Ka of a monoprotic weak acid is 5.8 x 10-6, what is the pH of a 0.12 M solution of this acid?

A: Negative logarithm of Concentration of [H+] ion present in the solution is known as pH of the…

Q: What is the pH of a solution when 25 ml, 0.200 M of salicylic acid CeH:(OH)COOH is diluted to 100.0…

A: Given: Concentration of salicylic acid i.e. HA (Assuming it HA as its monoprotic acid) = 0.200 M…

Q: Calculate the pH in the solution formed by adding 10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M…

A: The number of moles of benzoic acid and NaOH in the solution can be calculated using equation (1),

Q: If 34.6 mL of a 0.68 M NaOH solution is added to a 51.9 mL sample of a 0.68 M weak acid, HA , what…

A: 34.6 mL of a 0.68 M NaOH solution is added to 51.9 mL sample of a 0.68 M weak acid, HA (ka = 1.8 x…

Q: Calculate the pH of a 0.250 M aqueous solution of CH3COOH. alculate the pH of a solution having…

A: Given,  i) The molarity of aqueous solution of   CH3COOH = 0.250 M.  The pH of the solution is: ii)…

Q: What is the pH in the titration of 50 ml of a 0.150 M solution of KOH with 50.00 ml of 0.150 M HBr?

A: Volume of KOH=50 mL  Concentration of KOH=0.150M  Volume of HBr=50 mL  Concentration of HBr=0.150 M…

Q: what is the pH of a solution prepared by adding 63.6 mL of 0.100 M sodium hydroxide to 69.37 mL of…

A: Given that : The volume of sodium hydroxide = 63.6 mL The molarity of sodium hydroxide = 0.100 M The…

Q: Calculate the pH of a solution made by adding 0.123 g of solid NaOH to 275 mL of 0.350 M HNO2 (Ka =…

A:

Q: What is the pH in the titration of 50 ml of a 0.150 M solution of KOH with 15 ml of 0.150 M HBr?

A: Given  Volume of KOH = 50 ml = 0.050L Molarity of KOH = 0.150 M Volume of HBr = 15 ml = 0.015 L…

Q: What is the pH of the resulting buffer solution when 25mls of 0.10 M NaH is added to 25mls of 0.200…

A: pH of the buffer solution is calculated by using Henderson equation, it is,

Q: What is the pH in the titration of 50 ml of a 0.150 M solution of KOH with 55.00 ml of 0.150 M HBr?

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration of a solution expressed…

Q: If the K of a monoprotic weak acid is 1.8 x 10-6, what is the pH of a 0.35 M solution of this acid?

A: Given: Ka of weak monoprotic acid (Assuming HA) = 1.8 × 10-6  And the concentration of HA = 0.35 M

Q: In a titration experiment of a 25.00 mL of 0.100M CH3CO2H with 0.100 M NaOH, 12.50 mL of NaOH were…

A: Answer:- this question is answered by using the simple concept of calculation of pH of a weak acid…

Q: Calculate the pH of the solution formed when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of 0.100 M…

A: NaOH will react completely with acid CH3COOH as its a strong base NaOH + CH3COOH -------->…

Q: 20 ml of 0.2 M NaOH solution be treated with 40 ml of 0.2 M acetic acid solution to give 60 ml.…

A: An acidic buffer is defined as an aqueous solution that consists of a mixture of a weak acid and its…

Q: What is the pH of a sodium acetate (NaCH3CO2) solution prepared by adding 0.820 g of sodium acetate…

A: Given: Mass of sodium acetate = 0.820 g Volume of water             = 100.0 mL Ka of acetic acid…

Q: Calculate the pH of a buffered solution that is 0.100 M in C6H5COOH (Ka = 6.4 x 10–5) and 0.100 M in…

A: Given: C6H5COOH=0.100 M Ka=6.4×10-5 C6H5COONa=0.100 M To find: pH of buffered solution Solution: pH…

Q: Calculate the pH of the solution when 45.0 mL of 0.25 M HNO2 is mixed with 45.0 mL of 0.35 M NaOH.…

A:

Q: What is the pH for a weak monoprotic acid if a 0.020 M solution of the acid has a Ka of 3.28 x 10-7…

A: The H3O+ concentration for the weak acid is determined given below:

Q: Calculate [OH⁻] in a solution obtained by adding 1.70 g solid KOH to 1.00 L of 10.0 M NH₃. (Kb of…

A: Given Molarity of NH3 = 10M Mass of kOH = 1.7g Kb of NH₃ is 1.80 × 10⁻⁵ Molar mass of KOH = 56 g/mol…

Q: Calculate [OH⁻] in a solution obtained by adding 1.10 g solid KOH to 1.00 L of 10.0 M NH₃. (Kb of…

A: Given data,Mass of KOH=1.10gMolarity of NH3=10.0MVolume of solution=1.0LKb=1.80×10-5

Q: When a weak acid, HA, is titrated with a strong base, NaOH, what species are increasing in…

A:

Q: If a buffer solution is 0.100 M in a weak acid (K, = 5.7 x 10-5) and 0.530 M in its conjugate base,…

A: We have  0.1 M of weak acid of Ka 5.7*10-5 . Concentration of conjugate base as 0.53 M We have to…

Q: how you determine the pH when 15 ml of 0.100 M HCI is ado 080 M NH3 (K, = 1.6 x 10-6)

A: Given,  Kb = 1.6×10-6 pKb = -log(Kb) = -log(1.6×10-6) = 5.82 Molarity of HCl = 0.100 M Volume of HCl…

Q: What is the pH of a solution when 82.5 mL of a 0.1M HCN solution (ka = 6.2 x 10 -10) is titrated…

A: pH of a solution is the negative logarithm of the H+ ion concentration. In acid-base titrations, one…

Q: What will be the pH of a solution when 100.0 mL of 0.100 M NaOH is reacted with 9 mL of 1.00 M…

A: Applying formula MV=M1V1- M2V2  POH = -log [OH-]

Q: What is the pH of a solution that is 0.32 M H(C6H5COO) and 0.12 M Na(C6H5COO)?   The Ka of…

A: Answer:- This question is answered by using the simple concept of calculation of pH of solution…

Q: What is the pH of a mixture that contains 0.20 M Ca(OH)2 and 0.20 M LiOH?

A: Strong bases completely ionize when dissolved in water. Both the base, Ca (OH)2 and LIOH are strong…

Q: Benzoic acid (Ka=6.6 x 10^-5) is present in many berries. Calculate the pH and % ionization of a 593…

A: Concentration of solution can be calculated by the formula: Concentration = Number of moles of…

Q: Lemons get their sour flavor from citric acid (Ka = 7.4 x 10-4) a fresh squeezed lemon can have a…

A: Concentration of citric acid = 0.3 M  Volumeof citric acid = 20 ml  Concentration of KOH = 0.6 M…

Q: If you titrate 20.00 mL of 0.10 M HCI with 0.10 M NaOH, Calculate the pH after adding 24 mL of 0.10…

A:

Q: 75.0 mL solution of 0.800 mol/L hypobromous acid HBrO(aq) is being titrated with 1.25 mol/L Sodium…

A: Millimoles of acid=75*0.8= 60 Millimoles of base=1.25*48=60  So salt is formed . NaBro is formed…

Q: If a buffer solution is 0.240 M in a weak acid (Ka = 3.8 x 10-5) and 0.530 M in its conjugate base,…

A: Introduction Henderson - Hasselbalch equation gets used to calculate the pH for any buffer solution…

Q: Question is attached

A:

Q: When a weak acid, HA, is titrated with a strong base, NaOH, what species are increasing in…

A: Weak acid does not dissociate completely and the dissociation of the weak acid HA is given by: HA  ⇌…

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.