In a solution with a pH value of 7.0, hypochlorous acid a0 and Find the a1 values. (ka for HOCI= 3x10-8)

Q: Phosphoric acid, H3PO4 is a triprotic acid.    pKa1= 2.16      pKa2=7.21            pKa3=12.32…

A: Given data, Molarity of HPO42-=0.450MpKa1=2.16pKa2=7.21pKa3=12.32

Q: 2) A 0.10 M solution of which of the following salts would be predicted to exhibit a pH of 7.46 at…

A: Henderson Hasselbalch equation The equation that is used to calculate the pH of a buffer system is…

Q: Pentanoic acid is another example of a weak acid. d. Calculate the value of Ka for a solution of…

A: Given: Concentration of pentanoic acid = 0.05mol/L pH = 3.05

Q: A weak acid has a Ka = 5.78x10. What is its pK3? %3D 9.244 8.238 O 1.660 0.999

A: Given, the Ka for a weak acid = 5.78 × 10-9 We have to calculate the pKa of the acid.

Q: 27. Antacids are generally A. strong acids B. weak acids C. strong bases D. weak bases E. salts…

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Q: Complete the following table.   Acid Ka pKa A HNO2 4.5×10-4   B HClO 3.5×10-8   The weaker acid…

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Q: Calculate the pH of 4.0 X10*-4 M KOH O a. 9.40 O b. 3.40 O c. 4.60 Od. O d. 10.60

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Q: For each value of pKa, calculate the corresponding value of Ka. Which compound is the stronger acid?…

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Q: Given the weak acid, boric acid (H3BO3), calculate the pH and pOH of a 4M boric acid solution. Ka =…

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Q: Suppose Al(OH)3 is added to water until no more can be dissolved, giving rise to a solution with a…

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

Q: Which of the following acids is the weakest? hypoiodous acid (HIO) periodic acid (HIO4) iodous acid…

A: Since for an acid it has to be easy to release the H+ ions as soon as possible to be most strongest.…

Q: The acid-dissociation constants of phosphorous acid (H3PO3) are Ka1 = 7.5 x 10 3, Ka2 = 6.2 x 108,…

A: Dissociation constant are based on ion of H3PO3 .

Q: Identify which of the acids below will yield the stronger conjugate base and why. а) НОСI (К, — 3.5…

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Q: Identifying Acids and Bases. Write the formula of the conjugate acids of the following bases: a.…

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

Q: The pH of a 0.063-M solution of hypobromous acid (HOBr but usually written HBrO) is 4.95. calculate…

A: Given: pH of hypobromous acid, HOBr = 4.95 Concentration of HOBr acid = 0.063 M Ka = ?

Q: Calculate the pH of an aqueous solution of 0.70 M H3BO3 and 0.40 M H;BO3 Acid Formula Ka pKa HCOOH…

A: Henderson - Hasselbalch equation:

Q: Calculate the pH at 25 °C of a 0.46M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

A: Given data :

Q: According to the following pKa values listed for a set of acids, which would lead to the strongest…

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Q: Calculate the pH of a 0.0250 M solution of butanoic acid. Ka = 1.5x10-5 HC4H7O2(aq) +H2O(l) = H3O+…

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Q: 18. If 0.21 M solution of an acid (HA) has a pH of 2.0; then the Kb of the conjugate base (A-) of…

A: HA (aq) + H2O (l) ⇔A- (aq)+ H3O+(aq)

Q: Ka for ammonium, its conjugate acid. (NH4+) = 5.68 x 10^-10 Using the answer above, what is the pH…

A: Given: Ka = 5.68 x 10-10 Concentration of NH4Cl = 0.140 M

Q: Which chemical group is most likely to be responsible for an organic molecule behaving as a base…

A: The functional groups are the groups attached to a hydrocarbon chain that is responsible for their…

Q: The pH of a 0.59M solution of barbituric acid (HC,H,N,0,) is measured to be 2.12. Calculate the acid…

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Q: find [H3O+] in M ph=2.00

A: Given,  The pH of the solution is 2.00 The [H3O+] is:

Q: On acidity and basicity of aqueous solutions, the following relationships are valid, except…

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Q: 2. Given the following values for the apparent pH, find (H*) in the following solutions: (a) pH = 0…

A: The pH of any solution shows that the solution is acidic or basic.  For multipart questions, we are…

Q: If the pH of a 1.00 in. rainfall over 1700 miles^2 is 3.40, how many kilograms of sulfuric acid,…

A: Height of rainfall = 1.00 inch = 0.0254 m Area of rainfall = 1700 miles² 1 mile² = 2.59×10⁶ m²…

Q: weak Mandalorious acid (HMaO3): 4.5 x10-1 M, Ka = 6.7 x 10-5  Determine the pH of the solution

A: The acid dissociation constant for the HMaO3 is = 6.7×10-5 The concentration of HMaO3 solution is =…

Q: The diprotic acid H₂A has Ka1 = 1.58*10-5 and Ka2 = 1.47*10-6. If the initial concentration of H₂A…

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Q: Complete the following table. Acid Ka pK A HNO2 4.5x104 B HCIO 3.5x10-8 The weaker acid is

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Q: c. H20 = Lewis Base (donate 10. Calculate the pH of 0.3M solution of NH,Br if Ka of NH4* = 5.6x10-10…

A: The pH of a 0.3 M solution of NH4Br is to be calculated if Ka of NH4+ = 5.6×10-10

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: Solution -

Q: 2. Calculate the pH of a 0.200 M solution of H2SO4. Ka2 for H2SO4 is 1.2 x 102. (Since Kaz is high,…

A: Step -1  we know that  PH = -log(H+) H2SO4 - gives two H+ ions in dissociation condition. So, 2 x…

Q: 5. Which of the following is Lewis acid BF3 FeC12 AICI3 All of the above

A: According to the definition of lewis acid is that, Element,atom or ion having incomplete octet or…

Q: Find the a0 and a1 values ​​of hypochlorous acid in a solution with a pH of 7.0. (Ka = 3x10^-8 for…

A:

Q: 3- The pOH of a sample of baking soda dissolved in water is 5.74 at 25°C. Calculate the pH, [H'],…

A: PH and PH Scale :  Meaning of pH  is the power of hydrogen ion.  It is expressed as : pH = -log[H+]…

Q: Predicting acid or base strength from the conjugate species 0.1 M aqueous solution НСООН HC,04…

A: pH is used to determine the alkalinity or acidity of a reaction. The pH is determined as the…

Q: What is the pH of a 1.00*10-°M solution of KOH at 25 °C? 5.000 9.000 12.400 13.980 7.004

A: pOH= -log[OH-] = -log 10-9 = 9

Q: Find the pH of a 0.247 M NH4Cl solution given that the Kb of NH3 = 1.8x10-5 at 25 °C. 11.32 2.68…

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Q: Calculate the pH of a solution that is 1.8*10^-3 M morphine if the pKa of its conjugate acid is 8.21

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

Q: Calculate the pH of a 0.36M methylamine (weak base) (CH3NH2) solution, if Kb = 4.4x10-4   899 10…

A: The pH of a 0.36 M methylamine (weak base) (CH3NH2) solution is to be calculated, if Kb = 4.4x10-4.

Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00789 M…

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Q: Given Methylamine (CH3NH2). Calculate pH of a 0.0010 M solution of this base. Given Kb for CH:NH2 is…

A: As per guidelines if multiple q uestions , first question is allowed to answer , please post…

Q: What is the pH of a 0.2 M solution of sodium propionate C2H5COONA (salt) solution? (For propionic…

A: pH is the potential of the hydrogen atom, pH is a logarithmic function, it is found from the…

Q: Consider a weak acid "HA". What is the percent ionization of a 0.635 mol L-1 solution of HA? Just…

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Q: Sulfuric acid (H2SO4) has two acidic protons with the following ionization constants: Ka1 is…

A: As we know, Strong acid dissociates completely and releases [H+] ion. So, we can calculate directly…

Q: Caffeine (CHiON O2) is a weak base with a pKof 10.4. Calculate the pH of a solution containing a…

A:

Q: List the following by ability to ionize, least to greatest. HC7H5O2, Ka = 6.3x10-5 HC2H3O2, Ka =…

A: The higher the value of Ka, the higher will be the value of ions produced. Thus, the value of Ka is…

Q: Calculate the pH at 25 °C of a 0.85M solution of ethylammonium bromide (C,H,NH,Br). Note that…

A: The given data contains, concentration = 0.85 M. pKb= 3.19

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.