pH = 10.31 Use the following table to predict the best acid/ base pair for the desired pH/pOH values below (hint: remember buffer range = ± 1 pKa unit). Acid Base     Name Acid Base pKa Hydrochloric acid HCl Cl- -7.00 Phosphoric acid H3PO4 H2PO4- 2.12 Hydrofluoric acid HF F- 3.18 Lactic acid Lactic acid Lactate 3.85 Acetic acid CH3COOH CH3COO- 4.74 Carbonic acid H2CO3 HCO3- 6.36 Dihydrogen phosphate H2PO4- HPO42- 7.21 Ammonium NH4+ NH3 9.25 Hydrocyanic acid HCN CN- 9.31 Bicarbonate HCO3- CO32- 10.25 Methylammonium ion CH3NH3+ CH3NH2 10.62 Hydrogen phosphate HPO42- PO43- 12.38

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Q: Which weak acid would be best to use when preparing a buffer solution with a pH of 9.50? an acid…

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Q: Calculate the pH of a solution prepared by adding 30.0 mLs of 0.20 M HCl to 50.0 mLs of 0.10 M…

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Q: 6. Calculate the percent dissociation of 0.10 M hydrazoic acid (HN3, Ka= 1.9 x 10-5). Recalculate…

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Q: 1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka = 1.8 x…

A:

Q: == H2A is a diprotic acid with Ka1 = 5.42\times 10-5 and Ka2 = 3.76\times 10-10. Consider the…

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Q: Calculate the pH of 0.391 L of a 0.25 M acetic acid - 0.27 M sodium acetate buffer before (pH1) and…

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Q: You have an aliquot of 10 mL of 0.1022 mol/L phosphoric acid.  The ka values for phosphoric acid are…

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Q: f. 1.00 mL of 0.175M NaOH diluted to 375 mL (M₁V1 = M2V2) g. 5.00 x 10-³ M Ba(OH)2 solution h. 2.055…

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A:

Q: You have an aliquot of 12 mL of 0.1010 mol/L phosphoric acid.  The ka values for phosphoric acid are…

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Q: An acidic solution has a pH of 3.4 pH with an acid dissociation constant Ka of 4.0 X 10-7. What is…

A:

Q: Phosphoric acid is a triprotic acid with the Ka values of 7.25 10-3, 6.31 10-8 and 3.98 10-13…

A: Millimoles of H3PO4 taken   =Molar concentration of acid×Volume of acid=0.1000 M×25 mL=2.5 mmol

Q: You have an aliquot of 10 mL of 0.1094 mol/L phosphoric acid.  The ka values for phosphoric acid are…

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Q: As the strong reaction finishes, the concentration of conjugate base ion is 0.20 M. It then goes…

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Q: You mix 50.0 mL of 0.250 M CH3COOH with 1.00 mL of 0.500 M NaOH. Calculate the pH of the mixture.…

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A: Calculation as shown below

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Q: What is the pH (answer in 2 decimals) of a solution containing 0.25 M sodium formate (HCOONa) and…

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Q: 3, Calculate the pH of a solution prepared by mixing 150.0 mL of 0.200 M hydrobromic acid and 150.00…

A: (3)

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Q: Find the pH of a solution prepared by mixing 2.15 g of butyric acid (HC4H7O2) with 0.450 g of NaOH…

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A:

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Q: [HCl] 10-1 10-2 10-3 10-4 10-5 10-6 10-7 pH

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Q: Calculate the pH

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Q: 4-)

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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.