Calculate the pH of a sample of rainwater if it is left to equilibrate with 2.0 ppmv of SO2 (KH = 1.2 molL atm). Assume SO2 is the only acidic gas present. Given: KH (SO2)=1.2 mol L atm Kai (H2SO) = 1.7 x 10 mol K2 (H2SO;) = 6.6 x 10 mol

Q: A large volume of 0.1760 M H2SO3(aq) is treated with enough NaOH(s) to adjust the pH of the solution…

A: Introduction: pH: pH is used to express the acidity of the solution. It is defined as negative…

Q: 2. A 55-year-old patient was admitted to the hospital with shortness of breath and cough. Rapid…

A: A buffer is a solution that can hold the pH of the solution at a certain value when small amount of…

Q: Calculate the pH of a solution of 6.5 x 109 mol of Ca(OH)2 in 10.0 L of water. Ksp(Ca(OH)₂) = 6.5 x…

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Q: Calculate the pH of a 0.23 M sodium formate solution (HCOONA). Kp for HCOO = 5.9 x 10-11

A: Given that,    Concentration of HCOONa solution = 0.23 M   Kb for HCOO-  = 5.9×10-11  Since, pKb =…

Q: The reaction of an acid and a base only produces a salt and water as products. This is an example of…

A: When an acid(say HA) reacts with a base (MOH). They produce salt and water.

Q: 1. Determination of Vitamin C in Grape Juice acid, which gives the characteristic citrus taste to…

A: Citrus fruits contain Vit C. It is antioxidant that is essential for human body. Vit C content can…

Q: Calculate the pH of a solution of 6.5 x 10 mol of Ca(OH)2 in 10.0 L of water. Ksp(Ca(OH)₂) = 6.5 x…

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Q: Give an explanation of the solubility of Lithium Halides

A: Solubility of the species depends on the size of the ions, polarizability, covalent character and…

Q: A solution of H2SO4 is found to be 0.5172 N and 39.65 mL of it are equivalent to 21.74 mL of…

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Q: Calculate the pH of a solution that is prepared by dissolving 0.23 mol of hydrofluoric acid (HF) and…

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Q: The active compound in Pepto-Bismol contains C, H, O, and Bi.(a) When 0.22105 g of it was burned in…

A: Since we only answer up to 3 sub-parts, we will answer the first three. Please resubmit the…

Q: Calculate the concentration of CO²- In an aqueous solution of 0.255 M carbonic acid, H₂CO₂ (aq).…

A: Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.47*10-7 and Ka2 = 4.68*10-11  Given the…

Q: Calculate the pH, the pOH, and the molarity of all species in solution for a 6.15 M methylammonium…

A: We have asked to calculate pH, the pOH  and molarity of all species in solution. The answer to this…

Q: What is the pH of a solution prepared by dissolving 0.445L of HCl (g), measured at STP, in enough…

A: At STP conditions, 1 mole of any gas has the volume of 22.4 L. No. of moles in 0.445 L of the gas at…

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

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Q: A sample of water has a pH of 5.3. The concentration of bicarbonate (HCO3-) in the sample is 190…

A: The concentration of hydrogen ion and hydroxide ion in mg/L is; H+=10-5.3H+=10-5.3 mol/L×1g/mol×1000…

Q: Bacteria in the human mouth release enzymes to break up sucrose, and then polymerize glucose to form…

A: Given:       Ka of lactic acis = 1.38×10-4       Initial concentration of lactic acid =0.10 mol/L

Q: Estimate the pH of 0.010 M NaCH3CO2(aq).

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Q: Determine the pH of a 0.461 M C3H5CO,H M solution if the K, of C6H5CO2H is 6.5 x 105. 4.52 11.74…

A: pH  is commonly known power of hydrogen,  it measures the concentration of hydrogen ion in the…

Q: 3. Explain the differences in conductivity between: a) aqueous solutions of acetic acid…

A: We have to explain the conductivity  between the  following  solution

Q: The pH is measured to be 2.58 for a solution of 0.035 M cyanic acid, HOCN (aq). Write the hydrolysis…

A: HOCN is a weak acid. Weak acid are those acid which does not dissociates completely in equilibrium.…

Q: The base trimethylamine, (CH3)3N, has a pKb equal to 4.20. Calculate the hydroxide concentration,…

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Q: If 100.0 g of P,01, reacts with excess water to form 0.500 L of solution, what is the concentration…

A: Since you have asked multiple questions, we will solve first question for you. for any specific…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

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Q: i Calculate the pH, pOH, and fraction of solute protonated or deprotonated in the following aqueous…

A: Hello. Since the question contains more than three sub-parts, the first three sub-parts shall be…

Q: What is the pH of a 0.250 M solution of H2SO4? K22 = 1.20×10-2

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Q: A 1.2 · 102 M aqueous solution of Ca(OH)2 at 25.0 °C has a pH of, O 12.38 O 12.08 O 1.62 O 2.4 · 102…

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Q: Estimate the Ph of a .20M solution of CH3COOH with of Ka=1.8x10^-5

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Q: Why is rainwater naturally acidic, even in the absence ofpolluting gases such as SO2?

A: Acidic substances are those substances that have a pH value is in the range of 0 to 7. When the…

Q: The pH for a solution with a [H3O]+ of 1.0 x 10^-6 is

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Q: When ammonium acetate is dissolved in water, the following reaction takes place: NH,C,H,O2 (aq) - NH…

A: Given reaction:   NH4C2H3O2 (aq)   ----->  NH4+(aq)  + C2H3O2-(aq)  volume of 0.15 M NH4C2H3O2…

Q: Nitrous acid is a weak acid and has a concentration of 0.65 mol/L. What is the pH of the solution…

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Q: Complete and balance the following equations for reac- tions taking place in basic solution. (a)…

A: Redox reactions are the reactions in which oxidation and reduction occur simultaneously. Balancing…

Q: Fill in the left side of this equilibrium constant equation for the reaction of nitrous acid (HNO,)…

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Q: Calculate the pH of a dilute solution that contains a molar ratio of potassium acetate to acetic…

A: Henderson equation for acidic buffer solution: pH = pKa + log CH3COO-CH3COOH  (a) pH = 4.76 + log…

Q: An industrial sewage must be discharged into a receiving stream with a pH of 8,3 and alkalinity =…

A: Given:  When pH = 8.3 Carbonates = 100% HCO3 - Conc of [HCO3-] = 2 x 10-3 eq/L When pH = 6.3…

Q: he reaction of an acid and a base only produces a salt and water as products. This is an example of…

A:

Q: The sodium salt of propanoic acid, NaCH3CH2CO2, is used as an antifungal agent by veterinarians.…

A: Given: The Kb for CH3CH2CO2- = 7.7 × 10-10 We have to calculate the concentrations of H3O+ and OH-,…

Q: Human blood has a pH of approximately 7.4 due to the carbonic acid/bicarbonate ion (H2CO3/HCO3−)…

A: #(i): The given reaction for the dissociation of H2CO3 is  H2CO3(aq)  ⇌ CO2(g) + H2O(l)

Q: The first step in purifying the urine collected on the ISS is to treat every liter of urine with 20…

A: #(a): H2SO4 is a diprotic acid. The dissociation equations are: H2SO4(aq) ----> HSO4-(aq) +…

Q: What volume of 2.25-M H2SO4 should be diluted with water to form a 1.25 liters of 1.5 molar of the…

A: The process of dilution is defined as the process in which a solution with a lower concentration is…

Q: 2.50 g of sodium acetate, CH3COONa was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M…

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Q: Nitrous acid, HNO2 (aq) has a Ka value of 4.0 x 10-4. What is the pH and POH of a 0.0500 M solution…

A: The question is based on the concept of equilibrium. we have to determine PH and pOH   of weak acid…

Q: How many moles of hydroxide ions can be released into solution from 1.00 mg of Mg(OH)2 that is used…

A: Molar mass of Mg(OH)2 = 58.32 g/mol Given mass = 1 mg = 0.001g Moles = 0.001/58.32 = 1.71*10-5

Q: Selenous acid is a diprotic acid, for Ka1 = 9.43 x 10-3 and Ka2 = 7.39 x10^-8. Determine the…

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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.