Calculate the ratio [NH3]/[NH4+] in ammonia/ammonium chloride buffered solutions with the following pH values: a. pH = 9.00 b. pH = 8.80 c. pH = 10.00 d. pH = 9.60

Q: What is the pH of a solution containing 5ml of 0.1M NaOH mixed with 2ml of 0.15M HCl? a. None of…

A: Given Molarity of HCl  = 0.15 M Volume of HCl = 2 ml Molarity of NaOH = 0.1 M Volume of NaOH = 5 ml

Q: The weak acid HZ has a Ka of 2.55 x 10-4.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: Acid dissociation constant Ka is utilized to determine the acidic and basic nature of a solution. It…

Q: How many grams of NH4Cl (53.49 g/mol) must be dissolved in 0.612 L of solution in order to obtain a…

A: First we would Calculate molarity using pH and Ka value of NH4+ .  Them using molarity and volume we…

Q: 14.72 Acrylic acid (HC3H3O2) is used in the manufacture of paints and plastics. The pKa of acrylic…

A: The value of pKa of acrylic acid is 4.25. The concentration of acrylic acid is 0.150 M. The…

Q: how many moles of ammonium nitrate would be required to prepare .40 L of solution that is ph 5.40

A: NH3         +      HNO3     →       NH4NO3  weak base        strong acid            salt    Salt…

Q: The pKa for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.25 O b. 1.24 O c.…

A: this is the salt of weak acid and strong base. so ,we will use hydrolysis equation of weak acid and…

Q: Determine the pH of a 1.0M solution of sodium acetate (NaC2H3O2). Ka = 1.8x10-5 for acetic acid.

A: Dear student,  As you have asked multiple question but according to guidelines we will solve first…

Q: What is the pH of a solution that is 0.01M in picric acid and 0.1M in sodium picrate. (pKa=0.38)

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Q: Formic acid (HCHO,) has a K, 1.8 x 10. What is fractional composition (a) of formic acid in solution…

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Q: What is the pH of a solution that is 0.100 M NH3 and 0.350 M NH4CI? Kb of NH3 = 1.8 x 10-5 9.26 9.80…

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Q: An analytical chemist is titrating 164.9 mL of a 0.3400M solution of propylamine (C,H,NH,) with a…

A:

Q: Explain why the observed color change with bromcresol green for each of the four solutions is…

A: Since I am answering the first three sub-parts of multiple sub-parts. Please repost the question and…

Q: A. Identify the type of solution and calculate the pH for each of the following: i. 0.100 M HONH2…

A: PH = -log [H+] For weak acid [H+] = Kaweak acid Where [weak acid] is the concentration of the weak…

Q: Number 2 and 3 please! Thank you so much!

A: The acids that yield only a less quantity of hydrogen ions on dissolution are categorized under weak…

Q: How many grams of NH¼C1 have been dissolved in 300ml of 0.20 M NH3 to obtain a pH = 9.35? pKB= 4.75…

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Q: Q1/ Calculate the concentrations of the an ions species in (0.1 M H₂ASO4): [H], [OH'], [H₂ASO4],…

A: Since ka1 >>>Ka2 >>>> Ka3  so only first step is contributing in [ H+]

Q: 28. What is the pH of a 0.62 M NH;NO3 solution at 25 °C? * [Kb for NH, is 1.76 × 10*] A. 2.48 В.…

A: Ammonium nitrate is a slat of weak base, ammonium hydroxide and strong acid, nitric acid.…

Q: a) If a solution has a pH of 5.50 at 25°C, calculate its [OH]. b) The pH of a solution of HCl is 2.…

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Q: A solution contains 6.1 g/liter of benzoic acid. Calculate the pH. a. None of these O b. 1 С. 4 d.…

A: Here we have to determine the pH of aqueous solution containing 6.1 g/Liter of benzoic acid . Data…

Q: What is the pH of a solution of 12.01 g NaHSO4 (120.07g/mol) and 17.05 g Na2SO4 (142.05g/mol)…

A: The pH of a solution of 12.01 g NaHSO4 (120.07g/mol) and 17.05 g Na2SO4 (142.05g/mol) dissolved in…

Q: Calculate the pH of a 0.1 moldm³ solution sf a fully dissociated tribasic acid. 0.1 A 0.3 0.5 1.0…

A: Basicity of acid :-  The number of moles of  H+ ions provided by the dissociation of one of an acid…

Q: Calculate the ratio  in ammonia/ammonium chloride buffered solutions with the following pH values:…

A: A buffer solution is a solution that contains balanced amounts of weak acid and its conjugate base…

Q: Rank the following salts in order of increasing pH of 0.1 M aqueous solutions. (Hint: write out the…

A: We are given a combination of acidic, basic, and neutral salts.  Each salt has a concentration of…

Q: Calculate the pH of 100.00mL of 0.20 M HCIO4 solution after 124.00 mL of KOH 0.20 M have been added.…

A: Given that: Volume of HClO4 = 100.0mL = 100.0ml×1L/1000ml = 0.1L Molarity of HClO4 = 0.20M Molarity…

Q: 16.84

A: As, acid is formed, and base is precipitates. Therefore, the solution will be acidic.

Q: Calculate the pH of a solution made by 1 L buffered solution of 0.635 M NH3 with the addition of…

A: Given : volume of solution = 1 L  and concentration of NH3 = 0.635 M Hence moles of NH3 =…

Q: MasteringChemistry: CHE154 S X session.masteringchemistry.co This Mac can't connect to iCloud I a…

A: Concentration of OH- formed during the dissolution of NaF in water is determined as follows,

Q: HCN is a weak acid (?a=6.20×10−10) , so the salt, KCN , acts as a weak base. What is the pH of a…

A: First write down the reaction between KCN and H2O. Then find OH- or H3O+ and using that find pH of…

Q: Calculate the pH of the solution after the addition of each of the given amounts of 0.0554 M HNO3 to…

A: " Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: 7. Carbonic acid (H2CO3) is a diprotic acid with Ka1 = 4.30 × 10–7 and   Ka2 = 5.60 × 10–11 What…

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Q: Methane sulfonic acid, CH3SO3H (methanesulfonic acid) is a strong acid. Here is the reaction Of the…

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Q: Calculate the pH of a solution made by mixing 1.0mL of 3.0M NaOH with 40.0mL 0.20M H2CO3. The pKa1…

A: Pka = 6.35 For NaOH V= 1.0ml M= 3.0 M For H2CO3 V=40 ml M=0.20 M

Q: What mass of HI should be present in 0.250 L of solution to obtain a solution with pH value of 2.85.…

A: • Concentration = No. of molesVolume (L)• Mass = No. of moles × Molar mass• pH = -Log[H+}        ⇒…

Q: A buffer solution is 0.357 M in H2 C204 and 0.399 M in NaHC204. If Kal for H2 C204 is 5.9 x 10-2,…

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Q: What combination of substances will give a buffered solution that has a pH of 5.05? (Assume each…

A: The Henderson Hasselbalch equation for basic buffer is given as : Given, Volume of solution =…

Q: A chemist takes a liter of 1.25M H2SO4 and adds 1.50 moles of solid KOH. The addition of solid does…

A: The question is based on the concepts of PH calculation. we have been given sulphuric acid solution…

Q: C6H5NH2 + H2O C6H5NH3+ + OH-. Aniline, a weak base, reacts with water according to the reaction.…

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

Q: dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.39. A. Determine…

A: Introduction: A buffer solution contains a weak acid mixed with its conjugate base ,buffers resist…

Q: a) A solution consists of 0.15 M NH4Br and 0.18 M NH3. Calculate the pH of 1.00 L of the solution…

A: Buffers are solution that are used to resist the change in pH of the solution. They can be…

Q: 5. Determine the pH of the solution which has 10% of NaOH in deionized water by mass. The NaOH which…

A: Given that -  Mass percentage of sodium hydroxide, NaOH = 10%.  Density of this Solution = 1.131…

Q: What combination of substances will give a buffered solution that has a pH of 5.05? (Assume each…

A: The Henderson Hasselbalch equation for basic buffer is given as :

Q: A solution is made by dissolving 44.1 g of Ba(NO₂)₂ in 500.0 mL of water.   (a) Does Ba²⁺ have any…

A: Ba(NO2)2- is a salt . salt is made by reaction of an acid and a base . so this must be made from :…

Q: A chemist titrates 230.0 ml. of a 0.6154M ammonia (NH,) solution with 0.6407M HNO, solution at 25…

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Q: Calculate the values of [OH-] , and PH from Kb and [B initial]. Calculate the values of [OH-], POH…

A: NH3 dissociates as:                              NH3  +  H2O  ⇋  NH4+ +  OH-Initial mol…

Q: 2. If we mix 0.50 mol NaOAc and 0.50 mol HCIO into 1-L solution, the resulting solution should have…

A: Given: Moles of NaOAc mixed = 0.50 mol Moles of HClO mixed = 0.50 mol Volume = 1 L Kb(OAc-) =…

Q: 9. (a) What is the pH of () 0.10 М КОН (ад) (ii) 0.15 M HNO3(aq) (iii) The solution resulting from…

A: According to given problem, at first we have to calculate the pH values of a strong base (KOH), a…

Q: 1. a. Tris (C4H6(OH)3NH2) has a Ka of 7.94 x 10−9. Calculate the Kbfor this compound. b. If a…

A: 1. a. Given that : Ka of Tris (C4H6(OH)3NH2) = 7.94 x 10−9 We have to calculate the Kb for this…

Q: 36. Calculate the pH of each of the following buffered solutions. a. 0.50 M CH;NH/0.25 M C,H;NH;CI…

A: The question is based on the concept of PH calculations. we have been given three  solutions of…

Q: Calculate the pH of the following solutions: a) 400ml containing 7.5g Na2CO3 + 6g NaHCO3.

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions are…

Q: A solution of 0.10 M acetic acid and 0.10 M sodium acetatehas a pH of 4.76. Determine the pKaof…

A: Introduction: As per Bronsted-Lowry concept, an acid is a substance that can donate H+ ions and base…

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.