Consider a solution that is 0.046 M HF and 0.022 M NaF. 1) What is the pH of this solution? 2) What reaction occurs if H2SO4 is added? 3) What reaction occurs if KOH is added?

Q: An aqueous solution contains 0.464 M hypochlorous acid.How many mL of 0.364 M sodium hydroxide would…

A: The reaction between the sodium hydroxide and hypochlorous acid as shown below. At standard…

Q: An aqueous solution is prepared to be 0.221 M in sodium formate and 0.113 M in benzoic acid. (1) Is…

A: Solution:   (1):   Yes, it is a buffer solution. (2nd) and (3rd) part are solved in step no. 2 which…

Q: What is the ph of the solution that results when 25.0 ml of 0.125 M NaOH is added to 25.0 mL of…

A: I assume that you meant the 0.250 M HClThe balanced equation for the given reaction is,

Q: Determine the pH of a solution that is 0.15 M CH3COOH and 0.30 M CH3COONa.

A: GivenThe concentration of Acetic acid = 0.15MThe concentration of sodium acetate = 0.30M

Q: . The concentration of an unknown weak acid solution is 0.20M, and the solution has a pH of 3.89.…

A: Since you have posted multiple questions, we are entitled to answer the first only. Given: Initial…

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…

A:

Q: A buffer solution is 0.453 M in KH2PO4 and 0.271 M in K2HPO4. If Ka for H2PO4- is 6.2x10^-8, what is…

A: Buffer solutions show resistance to change its pH upon addition of strong acids or bases, which is a…

Q: Calculate the pH of a solution that is 0.60 M HF and 1.00 M KF.

A: Here HF is a weak acid, and F- is the conjugate base. Thus the solution having HF and KF is a buffer…

Q: 25 mL of a 0.356 M solution of NH4+ was mixed with 40 mL of 0.842 M potassium nitrate. What is the…

A: Given,  Molarity of NH4+ = 0.356 M  Volume of NH4+ = 25 mL  Molarity of KNO3 = 0.842 M  Volume of…

Q: An aqueous solution contains 0.464 M hypochlorous acid.How many mL of 0.364 M sodium hydroxide would…

A: The reaction as follows,

Q: Calculate the pH of a solution that is 0.0100 M in NaOH and 0.100 M in NH3.

A: Ammonia is a weak base and NaOH is strong base. Strong base ionize completely in the solution. Weak…

Q: The addition of Hf and ___ to water produces a buffer solution.  KOH KNO3 NaCI HBr NaBr

A: The solutions get prepared through mixing of weak acid+conjugate salt or weak base+conjugate salt…

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: In the laboratory, a general chemistry student measured the pH of a 0.598 M aqueous solution of…

A:

Q: If a buffer solution is 0.200 M in a weak base (Kb=7.4×10−5) and 0.450 M in its conjugate acid, what…

A: Calculate the pOH value of the given buffer solution,            pKb = - log Kb = -log (7.4 × 10-5)…

Q: What is the pH of a buffer solution with equal parts acetic acid and sodium acetate?

A:

Q: If a buffer solution is 0.200M in a weak acid (?a=9.0×10−5)and 0.550M in its conjugate base, what is…

A: Ka = 9.0 x 10-5  pKa = -log Ka = - log ( 9.0 x 10-5)  pKa = 4.046 [Acid] = 0.200 M  [Conjugate base]…

Q: How many moles of NH4Cl must be added to 2.0 L of 0.10 m NH3 to form a buffer solution with a pH of…

A: Formula used :-  . pOH = pKb + log[salt]/[base] . pH + pOH = 14

Q: Determine the pH if 25.0 mL of 0.20 M HI solution is added to 0.045 L of a 0.40 M KOH solution

A:

Q: An aqueous solution contains 0.494 M ethylamine (C2H5NH2). How many mL of 0.206 M hydroiodic acid…

A: Given data,Molarity of ethylamine=0.494MMolarity of HI=0.206MVolume of buffer=225mL=0.225LpH=10.6…

Q: A buffer solution contains 0.345 M NaHSO3 and 0.430 M Na,SO3. If 0.0273 moles of perchloric acid are…

A: We will use buffer equation

Q: A mixture of 100 ml of 0.025 M NH3 and 150 mL of 0.025 M NH4Cl was made. For this problem you need…

A: Number of moles of a chemical compound can be calculated by multiplying molarity of the solution…

Q: A buffer solution is 0.363 M in CH,COOH and 0.372 M in CH3COOK. If K, for CH,COOH is 1.8×10, what is…

A: Since CH3COOH is a weak monoprotic acid. And since the pH of monoprotic acid buffer is given by…

Q: If a buffer solution is 0.250 M in a weak acid (?a=2.3×10^−5) and 0.440 M in its conjugate base,…

A:

Q: If 0.25 moles of HCL were mixed with 0.25 moles of NaF (in 1.0 L final volume), what would be the pH…

A: pH can be calculated from the concentration of total H+ ions present in the solution. pH = - log…

Q: A buffer solution contains 0.222 M hypochlorous acid and 0.318 M sodium hypochlorite. If 0.0380…

A: Given buffer solution contains:  0.222 M hypochlorous acid(HClO) and 0.318 M sodium…

Q: A buffer solution is 0.080 M in lactic acid (Ka = 1.8 × 10−4) and 0.070 M in sodium lactate. The pH…

A: The pH of the buffer solution is find out using the Henderson-Hasselbalch equation. This equation…

Q: 50.0 mL of 0.100 M HBr(aq) is mixed with 50.0 mL of 0.0800 M KOH(aq). What is the pH of the final…

A: No. of mmol of HBr = 50 mL× 0.1M= 5mmol No. of mmol of KOH = 50 mL ×0.08M = 4 mmol

Q: A buffer solution is composed of 0.1 M CH3OOH and 0.2 M CH3COONA а.) What is the pH of this buffer?…

A: As per rule only three subparts of the first question can be answered. pH = pKa + log [salt] /…

Q: A buffer solution is 0.342 M in CH;COOH and 0.359 M in CH3COOK . If K, for CH,COOH is 1.8×10-5 ,…

A: Given: [CH3COOH] = 0.342 M [CH3COOK] = 0.359 M Ka of CH3COOH = 1.8×10-5

Q: A buffer solution is 0.390 M in H2 CO3 and 0.348 M in КНСОЗ. If Kal for H2 CO3 is 4.2 x 10-, what is…

A: Concentration of H2CO3 = 0.390 MConcentration of KHCO3 = 0.348 MKa1 of H2CO3 = 4.2×10-7

Q: A buffer solution contains 0.341 M ammonium bromide and 0.480 M ammonia. If 0.0405 moles of…

A: On addition of an acid to the basic buffer solution, the concentration of weak base decreases…

Q: What do you call an aqueous solution that has a large amount of NH4Cl and NH3 dissolved in it? Write…

A: a solution which resist in pH change value upon addition of small amount of strong acid or base…

Q: What is the pH if the hyrogen ion concentration in a vinegar solution is 0.001 M?

A: Formula Used pH = - log [ H+ ]

Q: There are 0.250 ml of a Buffer solution, where the concentration is 0.225 M of sodium acetate and…

A: In order to find the change in pH, we have to find both the initial and final pH.  Hence change in…

Q: You are given a 125 mL aqueous solution containing an unknown amount of NH4Cl salt. The solution has…

A: Given that, pH of solution =4.82  volume =125 ml =0.125 L  mass of NH4Cl =?

Q: Write a balanced chemical equation for the acid-base reaction that would occur if a small amount of…

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

Q: A buffer solution contains 0.254 M NaHSO3 and 0.348 M Na2SO3. If 0.0285 moles of hydroiodic acid are…

A: Calculate the initial pH of the given buffer solution using Henderson-Hasselbalch equation,

Q: What is the pH of a buffer solution that is 0.24M NH3 and 0.20M NH4Cl?

A: Given,Concentration of NH3 = 0.24 MConcentration of NH4Cl = 0.20 MAmmonia (NH3), is a weak base with…

Q: An aqueous solution is prepared to be 0.405 M in sodium fluoride and 0.261 M in acetic acid . (1) Is…

A: Given 0.405 M in sodium fluoride and 0.261 M in acetic acid . Add HBr 0.133 moles in 1L solution

Q: what is the pH?

A: Given :-  Concentration of weak acid = 0.250 M  Concentration of conjugate base = 0.450M  Ka = 5.9 ×…

Q: If 50mL of 0.10M NaOH is added to 50mL of 0.10M monoprotic weak acid, the resulting pH of the…

A: This can be calculated using Henderson -Hasselbalch equation

Q: What is the pH of a buffer solution that is 0.33 M propionic acid and 0.55 M sodium propionate?

A: Given: Concentration of propionic acid  = [C₃H₆O₂] = 0.33 M Concentration of sodium propionate =…

Q: 100 mL of 0.10 M HC1 is titrated with a solution of 0.10 M NAOH. After 20 mL of the NAOH solution,…

A: When acid and base react together and form salt and water this reaction is called a neutralization…

Q: What is the pOH of this solution?  What is the pH of this solution?

A:

Q: Calculate the pH of a solution that is 0.66 M HF and 1.00 M KF.

A: Given :- concentration of HF = 0.66 M                Concentration of KF = 1.00 M                Ka…

Q: A buffer solution is 0.302 M in Н2СОЗ and 0.305 M in NaHCOз. If Kal for На СОз is 4.2 × 10¬', what…

A: Henderson - Hasselbalch equation is:pH = pKa + log [Salt]/[Acid]                           . . . (1)…

Q: When someone blew into the flask that contained water with some universal indicator, and then shook…

A: Universal indicator:  Universal indicator is a mixture of several indicators produces different…

Q: Enough water was mixed with 1.26 g of sodium hydroxide (40.0 g/mol) to make a 500. mL solution. What…

A:

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.