A buffer solution is 0.384 M in H2CO3 and 0.328 M in KHCO3. If Kal H2 CO3 is 4.2 × 10-7, what is the pH of this buffer solution? pH =

Q: If a buffer solution is 0.230 M in a weak acid (Ka = 3.4 x 10-3) and 0.410 M in its conjugate base,…

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Q: When 0.412 g of a weak base with Kb = 3.10 ×10-5 the base is dissolved in 1.00 L of solution, it has…

A: Assuming the molar mass is M  Hence moles of base = mass / molar mass = 0.412 / M And concentration…

Q: A buffer solution is 0.320 M in H3PO4 and 0.254 M in KH2PO4. If Kal for H3PO4 is 7.5 × 10-3, what is…

A: H3PO4 is acid and KH2PO4 is a conjugate base of this acid. We use the Henderson Hasselbalch equation…

Q: Two acids are mixed in solution: 0.20 M of HBr and 1.50 M of HBRO (Ka = 2.3 x 10-9). What is the…

A: HBr is a strong acid while HBrO is weak acid and therefore, the resulting pH will be due to HBr,…

Q: A buffer solution is 0.486 M in NaH2PO4 and 0.394 M in Na, HPO4. If Ka for H2PO4¯ is 6.2 × 10¬8,…

A:

Q: Calculate the pH when 113.5 mL of 0.200 M HBr is mixed with 30.0 m

A: Given: the pH when 113.5 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 ×…

Q: If a buffer solution is 0.110 M in a weak base (K, = 1.9 × 10-³) and 0.480 M in its conjugate acid,…

A: Given that:  [Base] = 0.110M  [Salt] = 0.480M  Kb = 1.9×10-5 Pkb = -logKb = -log(1.9×10-5) = 4.72…

Q: What is the pH of a 0.220 M solution of sodium cyanide (NaCN)? Ka for HCN is 4.9 x 10-9.

A: NaCN has one less hydrogen and corresponds to a conjugate base (a weak base). The credentials…

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: A buffer, consisting of H2PO4- and HPO42-, helps control the pH of physiological fluids. Many…

A: The mass of NaH2PO4 is 6.5 g. The mass of Na2HPO4 is 8.0g. The Volume of the solution is 355 mL. We…

Q: If a buffer solution is 0.280 M in a weak base (K, = 5.7 x 10-5) and 0.450 M in its conjugate acid,…

A: We have to predict the pH of the solution.

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: 1. A buffer solution is 0.200 M in HC,H;O2, a monoprotic acid, and 0.200 M in NaCH,O2. K, for the…

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: The PH of 0.0296M HA ( Ka 8.4 *10-9) plus * . . 0.1026 M NaA is 4.3 2 O 8.6 7.5 O

A: The question is based on the concept of PH calculations. we have been given a weak acid and its…

Q: If a buffer solution is 0.170 M in a weak base (?b=3.7×10−5) and 0.540 M in its conjugate acid, what…

A: In question it is not mentioned whether the base is monoprotic or polyprotic. Hence assuming it 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: 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 solution that is 0.75 M HF and 0.15 M NaF?   The Ka of HF is 6.6 x 10-4

A: Given: Concentration of HF [HF]= 0.75 M Concentration of NaF [NaF]= 0.15 M Ka of HF is 6.6 x 10-4 To…

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: Malonic acid, HOOC CH2 COOH, can be used in a buffer system. What is the pH of a solution that…

A: A system containing Na+ -OOC CH2 COOH and Na+ -OOC CH2 COO-Na+ will act as as acidic buffer solution…

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: 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: A buffer solution is 0.308 M in H2 C204 and 0.252 M in NaHC204. If Kal for H2C2O4 is 5.9 x 10¬ª,…

A: The pH of a buffer solution prepared by mixing a weak acid with the salt of its conjugate base can…

Q: If the K of a monoprotic weak acid is 1.4 x 10-6, what is the pH of a 0.14 M solution of this acid?…

A: Given : Ka of monoprotic acid (assuming HA) = 1.4 X 10-6  And Concentration of acid = 0.14 M Since…

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: 100.0 mL of a 0.200 M H3PO4(aq) solution is titrated with 325.0 mL of a 0.100 M NaOH(aq) solution.…

A:

Q: A 1.00-L solution is made from 0.130 moles of C6H5NH2 (Kb = 3.9 × 10–10) and 0.170 moles of…

A: Given data,Moles of C6H5NH2=0.130molesMoles of C6H5NH3Cl=0.170molesVolume=1.00LKb=3.9×10-10

Q: A buffer solution is 0.372 M in NaHC204 and 0.323 M in Na2C₂O4. If K₂ for HC204 is 6.4E-5, what is…

A: Given: Concentration of NaHC2O4 is 0.372 M Concentration of Na2HC2O4 is 0.372 M Ka is 6.4×10-5 To…

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: A buffer solution is 0.328 M in H₂C2O4 and 0.275 M in NaHC204. If Ka for H₂C₂O4 is 5.9E-2, what is…

A: In this question, we need to determine pH of the solution. Here given the values of concentration of…

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: A solution prepared by mixing 1.73 of propionic acid (HC3H5O2) and 0.53 g of NaOH in water (Ka…

A:

Q: Calculate the pH of a 0.10-M solution of aluminum chloride, which dissolves completely to give the…

A: The hydration of aluminum chloride to furnish [Al(H2O)6]3+ ion is expressed as follows:…

Q: If the Ką of a monoprotic weak acid is 1.4 × 10-6, what is the pH of a 0.42 M solution of this acid?…

A: Given data, ka = 1.4 × 10-6  Concentration of Weak acid = 0.42 M

Q: Determine the pH of a solution made by adding 0.30 mol of acetic acid (CH3COOH) and 0.30 mol of…

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: A buffer solution is 0.416 M in H2 S and 0.245 M in NaHS. If K for H2S is 1.0 x 10-7, what is the pH…

A: This question is checking our basic concept regarding "Handerson - Hasselbalch equation".  We have…

Q: If the Ka of a monoprotic weak acid is 1.3 x 10-6, what is the pH of a 0.18 M solution of this acid?…

A:

Q: If the Ka of a monoprotic weak acid is 1.6 x 10-6, what is the pH of a 0.37 M solution of this acid?…

A:

Q: What will the pH be when you dissolve the following salts in water? Will the pH be acidic, neutral,…

A: A basic solution is the one in which the concentration of hydroxide is more than the concentration…

Q: The Ka of hypobromous acid, HOBr, is 2.6 x 10-9. Calculate the pH of a solu tion which is composed…

A: PH of acidic buffer can be calculated as follows

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: Q.6. A buffer is prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of…

A: Henderson Hasselbalch equation for buffer: pH = pKa + log ([salt] / [acid])

Q: A 0.381-M aqueous solution of NH3 (ammonia) has a pH of 11.4. Calculate the pH of a buffer solution…

A:

Q: Consider a solution that is 0.046 M HF and 0.022 M NaF. 1) What is the pH of this solution? 2) What…

A: Given: Concentration of HF = 0.046 M And concentration of NaF = 0.022 M

Q: Calculate the pH of a formic acid (Ka = 1.8 x 10-4) buffer solution that contains 0.35 mol HCOOH and…

A: Given:  Moles of HCOOH present = 0.35 mol Moles of HCOO- present = 0.28 mol Volume of the solution =…

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.