Calculate the pH of a 0.20 M solution of NH4NO3 Kb(NH3) = 1.8x10^-5 Thank you :)

Q: 32. Lactic acid (HC3H,O3) is a common constituent of a biologic systems. For example, it is found in…

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Q: Citric acid, which is present in citrus fruits, is a triprotic acid. (a) Calculate the pH of a 0.040…

A: Citric acid- It is weak organic acid. Dissociate in water as,

Q: . Strychnine, C,H„N‚O, (aq) is a weak base but powerfully toxic. (a) Calculate the pH of 0.001 mol/L…

A: Given: Concentration of weak base (assuming B) = 0.001 M And Kb of base = 1.0 × 10-6

Q: (a) Acid rain is no threat to lakes in areas where the rock is limestone (calcium carbonate), which…

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Q: Calculate the pH of a solution that is 0.0729 M LiC2H3O2 at 25°C.

A: LiC2H3O2 ( Lithium acetate) is the salt of a weak acid and strong base.   LiC2H3O2 → CH3COO- +…

Q: Calculate pH of the following solutions: a) 0.25 M HNO3 in 0.065 M CH3COOH (K,=1.75x10). b) 0.33 M…

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Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00577 M HCIO4 pH = (b) 0.523…

A: a) pH of a solution of 0.00577 M HClO4​ (perchloric acid)pH=−log ​[H+]In the case of a strong acid…

Q: The pH of a 0.0068 M solution of Ca(OH)₂ is

A: pOH = - log[OH-] pH + pOH = 14

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00357 M HIO4 pH =  (b)…

A: Note: As per our guidelines, we are supposed to answer only three subparts. Please repost the other…

Q: Consider the following ions: Cl-, HS-, NO2-, F-, and HS04-. (a) Which of these ions in water gives…

A: Given ions  Cl- HS- NO2- F- HSO4-

Q: The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid. (a) You are…

A: The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid.  (a) You…

Q: (a) The hydroxide ion concentration in an aqueous solution of NaOH is 0.10 M. Calculate [H3O+], pH,…

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Q: 1) A conjugate acid is defined as 2) In the general ionization reaction: HX(aq) + H,0(1) H,0* +…

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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 certain solution was found to have a pH of 5.50. Which of following statements is true about this…

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Q: Calculate the pH of each of the following strong acid solutions. (a) 0.000726 M HClO4 pH =…

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Q: The graph given below shows [H+] versus concentration foran aqueous solution of an unknown…

A: a) Since the concentration of H+ i.e [H+] is increasing with increase in the concentration of…

Q: Calculate the pH of a solution that is 0.0736 M KC2H3O2  at 25°C.

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Q: a) The average pH of normal arterial blood is 7.40 at 37° C. Calculate [H] for blood at this…

A: a) Given : pH of blood = 7.40

Q: The pH of 0.0720M solution of a weak acid is 2.670. What is the Ka of the acid

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Q: The pH of saliva is normally in the range of 6.4 to 7.0. However, when a person is ill, the person's…

A: pH is defined as negative logarithm of hydrogen ion concentration   pH= -log[H+] If pH<7 then the…

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00251 M HIO4 pH =  (b)…

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Q: Calculate the pH of the following solutions.(1a): 7.5 x 10-2 M HCl(1b): 0.0062 M KOH(1c): 2.84 g…

A: Hi there! Since this question contains multiple parts so I am answering the first three parts.

Q: Sodium hypochlorite solution is also known as bleach. It contains the hypochlorite ion ClO-.  (a)…

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Q: When answering this problem, report the answer with the appropriate number of significant figures…

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Q: The pH of a 0.0062 M solution of Ca(OH)₂ is

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Q: the pH and concentrations of species the following sõlutions (a) 0.20 M K,HPO4 An amphiprotic…

A: Amphiprotic species   Amphiprotic species can act both as acid and base by donating or accepting…

Q: - pH of Saliva The pH of saliva is normally in the range of 6.4 to 7.0. However, when a person is…

A: The acidic saliva indicates that the bacteria present in mouth breaks down the consumed carbohydrate…

Q: The pH of a solution of 0.50 M  NH4Cl  is

A: NH4Cl dissociates as follows: Ka of NH3 is 5.6×10-10 Thus concentration of HCl is 1.67×10-5 M.

Q: Calculate the pH of each of the following solutions. (a) 0.109 M HONH, (Kb = 1.1 × 10-8) 4.0 9.34 x…

A: The concentration of HONH2 = 0.109 M The concentration of HONH3+ = 0.109 M

Q: A student needs a sample of 0.772539887245 M NaOH for a laboratory experiment. Calculate (a) the…

A: It is given that the concentration of sodium hydroxide (NaOH) sample is 0.772539887245 M, the…

Q: The pH of a 0.0063 M solution of Ca(OH)₂ is

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Q: 7. Calculate [H3O+] and [OH-] for each solution of either a strong acid or a strong base. Calculate…

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

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00751 M HIO4 pH = (b)…

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Q: Determine the pH of the solution

A: According to question Ka = 1.82 x 10-⁵ Mass of acetic acid = 20.0 g Molar mass = 60.05g/mol  No. Of…

Q: In industrial environments, benzoic acid, C6H5COOH, is widely used to produce a range of products…

A: Given ,

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.