What is the hydronium-ion concentration of a 0.25 M solution of HCN (Ka = 4.9 × 10–10) at 25°C?

Q: acid

A: We know that acrylic acid is a weak acid therefore it will dissociate partially in the solution. The…

Q: What is [H⁺] in a 0.470 M solution of acrylic acid, CH₂CHCOOH (Ka = 3.16 × 10⁻⁵)?

A: Given values-> Molarity of H^+ = 0.470M Ka = 3.16 × 10^-5

Q: What is the percent ionization of a monoprotic weak acid solution that is 0.159 M? The…

A: According to the Arrhenius theory,an acid is a compound that when dissolved in water would furmish…

Q: What is the hydronium concentration of a 0.50M solution of hydrocyanic acid if the Ka at room…

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Q: What is the pH of a 0.680 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?

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Q: Calculate the pH of a 3.39×10-3 M  solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

A: Given : Concentration of NaF = 3.39 X 10-3 M And Ka of HF = 6.80 X 10-4  Since the salt NaF contains…

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Answer: NH4Cl is the salt of weak base and strong acid, therefore its hydrolysis will take place in…

Q: What is the percent ionization of a monoprotic weak acid solution that is 0.171 M? The…

A: We will first construct the ICE table. It will help us to write the equilibrium expression of the…

Q: What is [H+] in a 0.430 M solution of acrylic acid, CH₂CHCOOH (Ka = 3.16 × 10-5)?

A: We know that acrylic acid is a weak acid therefore it will dissociate partially in the solution. The…

Q: What is [H⁺]

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Q: What is the pH of the aqueous solution of an 0.25 M NaBrO solution Ka HBrO)= 2.0x10^-9

A: pH of an aqueous 0.25 M NaBrO solution.and   Ka (HBrO) = 2.0 × 10-9So,

Q: What is the pH of a 0.750 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?

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Q: What is the percent ionization of a monoprotic weak acid solution that is 0.1190.119 M? The…

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Q: Acetylsalicylic acid (aspirin), HC₉H₇O₄, is the most widelyused pain reliever and fever reducer.…

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Q: What is the equilibrium hydronium ion concentration of an initially 4.9 M solution of hypobromous…

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Q: NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: The ionization of NH4Cl as follows,

Q: The compound dimethylamine, (CH3),NH, is a weak base when dissolved in water. Write the K expression…

A: The ionization of weak base can be given by, Where B is the weak base and HB+ is its conjugate…

Q: What is the PH of a 0.13 solution of the salt NaX? Ka of HX= 1.5×10^-5

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Q: Calculate the pH of a 3.12×10-3 M  solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

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Q: What is the percent ionization of a monoprotic weak acid solution that is 0.165 M? The…

A: Interpretation -  To determine the percent ionization of a monoprotic weak acid solution that is…

Q: What are the concentrations of hydrogen ion and hydroxide ion in household ammonia, an aqueous…

A: The hydrogen ion concentration in aqueous solution of NH3 is calculated as shown below. on…

Q: Sodium fluoride is added to many municipal water supplies to reduce tooth decay.   Calculate the pH…

A: The dissociation of NaF is given as- NaF →Na++F− The concentration of NaF, [NaF]=3.39 ×10-3…

Q: molarity

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Q: percent ionization

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Q: What is the percent ionization of a monoprotic weak acid solution that is 0.1020.102 M? The…

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Q: Calculate the pH of a 0.400M solution of phosphoric acid, H3PO4.     Ka = 7.11*10^-3

A: Given: Concentration of H3PO4 = 0.400 M And Ka of H3PO4 = 7.11 × 10-3  NOTE: Since only the 1st Ka…

Q: Calculate the pH of a 3.97×10³ M solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

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Q: What is the pH of a 0.380 M solution of NACN (Ka of HCN is 4.9 x 1010)?

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Q: What is [H⁺] in a 0.260 M solution of acrylic acid, CH₂CHCOOH (Ka = 3.16 × 10⁻⁵)?

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Q: Arrange the following 0.10 M solutions in order of INCREASING pH (less acidic): HI, NaI, HF, NaF

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: What is the pH of a 0.780 M solution at 25 oC?   (  Ka = 4.9 x 10−10, at 25 oC)

A: Given, concentration of a solution (c) = 0.780M dissociation constant of acid (Ka) = 4.9×10-10

Q: What is [H⁺] in a 0.310 M solution of acrylic acid, CH₂CHCOOH (Ka = 3.16 × 10⁻⁵)?

A: Molarity of acrylic acid = 0.310 M  Ka = 3.16 × 10-5  [H+] = ?

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Q: Calculate the pH

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Q: What is the pH of a 0.750 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?

A: pH is the negative logarithm of hydrogen ion concentration. It can be given as pH=-log [H+]   NaCN…

Q: What is the percent ionization of a monoprotic weak acid solution that is 0.1380.138 M? The…

A: 0.138 M weak monoprotic acid solution has an acid -dissociation or ionization constant, Kaof 4.92…

Q: What is the percent ionization of a monoprotic weak acid solution that is 0.138 M? The…

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Q: HCIO is a weak acid (Ka=4.0*10^-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: At 25° C strength of NaOCl is 0.018 M and given Ka of acid is 4×10-8  We have to calculate the pH of…

Q: What is the pH of a solution consisting of 0.584M HF acid and 0.425NaF. The K a of HF is K a =6.6x10…

A: The answer is given as follows

Q: If the ph of a 30.0 mL sample of 1.0 M HOAc is 2.40 what's the equilibrium [H+] and the Ka value?

A: HOAc is a weak acid also known as acetic acid. The pH of a solution is related to the concentration…

Q: What is [H+] in a 0.270 M solution of acrylic acid, CH₂CHCOOH (Ka = 3.16 × 10-5)?

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Q: NH3 is a weak base ( ?b=1.8×10−5 ) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Ammonium chloride (NH4Cl) is a salt of a weak base (NH3) and a strong acid (HCl).When NH4Cl…

Q: What is the ph of a 0.0320 M solution of hydrocyanic acid HCN (Ka=4.9×10^-10)

A: Given : Concentration of HCN = 0.0320M

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.