A buffer solution is 0.467 M in HCIO and 0.321 M in NaCIO . If K, for HCIO is 3.5x10-8 , what is the pH of this buffer solution?

Q: A buffer solution is made that is 0.389 M in HCN and 0.389 M in NaCN. If K, for HCN is 4.00 x 10-10…

A: (a) Given that : The molarity of HCN = 0.389 M The molarity of NaCN = 0.389 M The Ka of HCN is 4.00…

Q: What is the pH of a buffer solution containing 0.21 M HNO2 and 0.10 M NO, ?

A: Since HNO2 is a weak monoprotic acid with pKa = 3.15  And the solution is given buffer solution with…

Q: A solution of is known to contain 0.100 M pyridine and 0.300 M pyridinum hydrochloride. The Kb for…

A: The determination of H+ ions which are available in any specific solution is carried out with the…

Q: A buffer solution is made that is 0.360 M in HNO2 and 0.360 M in KNO2. If K, for HNO2 is 4.50 ×…

A:

Q: A buffer solution is prepared from a generic weak acid "HG" and the salt KG. The K, for HG is 3.7 x…

A: Buffer solution is a solution that maintains and nullifies a small change in the pH of solutions. It…

Q: A buffer solution is made that is 0.397 M in HCN and 0.397 M in KCN. If K, for HCN is 4.00 x 10-10,…

A: Acidic buffer pH = pKa + log[salt]/[acid]   pKa = - logKa        = - log4 x 10-10        = 10- log…

Q: A buffer solution is 0.486 M in HF and 0.299 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…

A: Given :-  concentration of HF solution = 0.486 M  concentration of KF = 0.299 M  Ka for HF =…

Q: A buffer solution is 0.396 M in HF and 0.233 M in KF. If Ka for HF is 7.2x10-4, what is the pH of…

A:

Q: A buffer solution is made that is 0.355 M in HCN and 0.355 M in KCN. If K, for HCN is 4.00 x 10-10,…

A: We have to find the pH of the given buffer solution

Q: The K, for ammonia is 1.8 X 10 5. How many mL of a 0.70 M NH4CI solution is need when mixing with…

A: Given : Concentration of NH4Cl = 0.70 M Concentration of NH4OH = 1.0 M Volume of buffer = 50.0 mL…

Q: A 1.50 L buffer solution is 0.250M in HF and 0.250 M in NaF. Calculate the pH of the solution after…

A:

Q: Consider a buffer made with 3.4 mL of 0.35 M of a weak acid solution and 8.7 mL of 0.54 M solution…

A: given Ka = 9.3×10-4pKa = -log KapKa = -log  9.3×10-4pKa = 3.0315

Q: Consider a mixture of 1.36 M HCIO and 1.65 M NaCIO. Given that the K, for HCIO = 2.9 x 10-8…

A:

Q: A buffer solution is made that is 0.427 M in HNO2 and 0.427 M in KNO2. If K for HNO, is 4.50 x 10,…

A: Given-> Concentration of HNO2 = 0.427 M Concentration of KNO2= 0.427 M Ka(HNO2) = 4.50 × 10-4…

Q: A 22.3 mL sample of 0.344 M ethylamine, C2H5NH2, is titrated with 0.364 M perchloric acid. After…

A: Given,  Volume of C2H5NH2 = 22.3 mL  Molarity of C2H5NH2 = 0.344 M  Molarity of HClO4 = 0.364 M…

Q: 00 grams Ca(NO,), is placed in a 1150.ml 0.015M NH, ut of solution? What is the pH of the solution?…

A:

Q: A buffer solution is prepared by dissolving 1.000 g of ammonium chloride (NH,CI) into 100.00 mL of a…

A:

Q: A plot of pH vs volume of 0.05 M NaOH solution was obtained for titrating 0.4055 g of a dried solid…

A:

Q: When 50mL of 0.10 M  HOAc is titrated with 25mL of 0.1O M NaOH, the pH is

A: Given, Volume of acetic acid = 50mL. Concentration of acetic acid = 0.10M. Volume of NaOH = 25mL.…

Q: A buffer solution is made that is 0.401 M in HCN and 0.401 M in KCN. If Ka for HCN is 4.00 x 10 0,…

A: A buffer solution is made of a weak acid ie. Hydrocyanic acid (HCN) and potassium cyanide (KCN). pH…

Q: You want to prepare a buffer solution with pH equal to 3. How many grams of NaF (41.99 g/mol) should…

A: In this, we need to find oute moles of NaF first. Using that moles and molar mass for NaF, calculate…

Q: 200 M solution of HF to make a buffer with a pH of 3.00? (Ka for IF is 6.8 x 10-4)

A: Buffer is a weak acid and acid conjugate with strong base. Use acidic buffer equation to get the…

Q: A buffer solution is 0.422 M in HCN and 0.268 M in NaCN . If Ka for HCN is 4.0×10-10 , what is the…

A: Calculate the value of pKa:

Q: A buffer solution is made that is 0.301 M in H2S03 and 0.301 M in KHSO3. (1) If K for H2SO3 is…

A:

Q: The pH of a buffer solution that is made by mixing 124 mL of 0.156 M of acetic acids (pls=4.74) with…

A:

Q: A buffer solution is made that is 0.460 M in HCN and 0.460 M in NaCN. If Ka for HCN is 4.00 × 10¬10,…

A:

Q: A buffer solution is 0.405 M in HF and 0.200 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…

A: Here given, Concentration of HF = 0.405 M Concentration of KF = 0.2 M Ka for HF = 7.2 x 10-4 We…

Q: Question 2 I'm not sure how to do this problem

A: Assume 1L of solution Adding 8g of NaOH  Moles of NaOH added = 8/40 = 0.2 moles

Q: Which of the following statement is incorrect regarding buffer solutions: Maximum buffer capacity is…

A: Buffer solution are the mixture of acid and base or acid and its congugate base , it resist the…

Q: A buffer is prepared by adding 35 mL of 0.100 M hypochlorous acid, HOCl, to 65 mL of 0.300 M…

A:

Q: A buffer solution is 0.451 M in NaH PO, and 0.270 M in Na HPO4. If K, for H,PO, is 6.2x10, what is…

A: Henderson-Hasselbalch equation:- pH = pKa + {log[conjugate base]/[weak acid]}

Q: What is the pH of buffer that is 0.175 M in a weak acid and 0.200 M in the acid's conjugate base?…

A: Given data, Molarity of weak acid=0.175MMolarity of conjugate base=0.200MKa=5.7×10-4

Q: A buffer solution of 200 mL is prepared from 0.028 mol of a weak HX acid and 0.0070 mol of NaX.…

A: Buffer solution :- A solution which resists change in its pH value by the addition small amount of…

Q: A 24.4 mL sample of 0.211 M ethylamine, C₂H5NH₂, is titrated with 0.343 M hydroiodic acid. At the…

A: Ethylamine, C2H5NH2 is a weak base with pKa = 10.8  Ethylamine, C2H5NH2 when reacts with the strong…

Q: A 29.4 mL sample of 0.208 M triethylamine, (C,H3)3N, is titrated with 0.235 M hydrobromic acid.…

A:

Q: Calculate the pH of a carbonate buffer system that contains 0.0065 M HCO, and 0.0084 M CO,. The K,…

A: Given,  Concentration of weak acid, HCO3- = [HCO3-] = 0.0065 M  Concentration of conjugate base,…

Q: A buffer solution is 0.384 M in H2S and 0.210 M in KHS. If Kal for H2S is 1.0 × 10-7, what is the pH…

A:

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 is 0.437 M in HCN and 0.236 M in KCN . If K, for HCN is 4.0×10-10 what is the pH…

A: The Henderson-Hasselbalch equation gives the pH of buffer solution it is mathematically represented…

Q: A buffer solution is made that is 0.463 M in HF and 0.463M in NaF (1) If K for HF is 7.20×10, what…

A: USING the equation for pH of buffer , we can calculate the pH.

Q: A 200 mL buffer solution is prepared from 0.028 mol of a weak HX acid and 0.0070 mol of NaX. Since…

A: A mixture of weak acid (HX)  and its salt (NaX) with strong base acts as acidic buffer solution. For…

Q: A buffer solution is made that is 0.307 M in HCN and 0.307 M in KCN. If K, for HCN is 4.00 × 10¬10,…

A: A buffer solution is formed when a solution contains a weak conjugate acid-base pair. The given…

Q: A buffer solution is 0.402 M in H2CO3 and 0.314 M in KHCO3. If Kal for H2CO3  is 4.2 X 10 -7 , what…

A:

Q: For the buffer system in Problem no. 1, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b)…

A:

Q: An buffer is prepared by combining 4 L of a 0.57 M X solution with 4 L of an 0.57 molar HXCI…

A: Weak base are those base which does not dissociate completely in aqueous solution. Here X is weak…

Q: A buffer solution is made that is 0.329 M in HF and 0.329 M in KF. If K, for HF is 7.20 x 10 what is…

A:

Q: A buffer solution is made that is 0.376 M in HCN and 0.376 M in NACN. If Ka for HCN is 4.00 x 10-10,…

A: Hello. Since the question contains multiple parts, the first part is solved. In case the solution…

Q: A buffer solution is 0.441 M in HF and 0.245 M in NaF . If Ka for HF is 7.2×10-4 , what is the pH of…

A: Given, concentration of HF , [HF] = 0.441 M            concentration of NaF, [NaF] = 0.245 M…

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)…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.