A 2.14-g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution. The solution pH is 11.32. What is Kb for the hypoiodite ion?

Q: What mass ofn HNO3 is present in 285.0 mL of a nitric acid solution having a pH of 4.39? Mass =…

A: The answer to the following question is- Given, Volume of solution = 285 mL pH= 4.39

Q: The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of…

A: Given:Ka of H2CO3 is 4.4 ✕ 10−8

Q: A solution is prepared by dissolving 4.50 g of solid NaOH in 1.00 L o 0.100 M HNO₂(aq) (Ka =…

A: The pH of the solution can be calculated as follows

Q: 12.9 g of NaOH was dissolved in water affording a final volume of 250 mL. What is the pH of the…

A: Given :-  mass of NaOH = 12.9 g  volume of solution = 250 mL  To calculate :-  pH of solution

Q: how many moles of ammonium nitrate would be required to prepare .40 L of solution that is ph 5.40

A: NH3         +      HNO3     →       NH4NO3  weak base        strong acid            salt    Salt…

Q: A solution of 0.00100 M HCI has a pH of: (HCl is a strong acid and dissociates completely in…

A: Given that, Concentration of HCl acid = 0.00100 M Since, HCl is a strong acid, it completely ionised…

Q: You have a 1.25 L solution with 2.14 g of NaIO and the pH is 11,32. What is the Kb of NaIO?

A: Solution pH, pKa, pKb, Ka, and K ar employed in chemistry to explain however acidic or basic an…

Q: solution

A: KClO is a salt because it is formed from KOH strong base and weak acid HClO.  Weak part in salt…

Q: What is the pH of a 0.0520 M solution of HONH,CI (Kb of HONH, is 1.1 × 10*)? 2

A: Solution :      Weak bases show partial ionization on dissociation in an aqueous solution. Here…

Q: contains

A: For calculating the pH, we can used Hinderson equation,  pH = pKa + log( [salt] / [ acid ] )  Where…

Q: Suppose 0.100 mol of NaCH3COO is dissolved in enough water to make 1.00 L of solution. What is the…

A: pH is referred to the potential of hydronium ion and is calculated by taking the negative log value…

Q: The pH of the 0.50 M solution of HA is 1.92. What is [HA]?

A: Answer:pH is equal to negative of logarithm of hydrogen ion concentration in solution, so,

Q: 12 . What is the expected pH of a 0.015 M solution of boric acid (assuming 100% dissociation) ?

A:

Q: 7. What are the conjugate base and conjugate acid for HSO, ? What is the term used to describe…

A: Conjugate acid is formed when we add protons to a base and conjugate base is formed when proton is…

Q: A solution has a hydroxide-ion concentration of 0.043 M. What is its pH?

A:

Q: The pH of an aqueous solution of 9.43x102 M tellurous acid, H,TeO3 (aq), is For H,TeO3 K =5.40*10…

A: Dissociation of tellurous acid is, Ka1 and Ka2 values of a tellurous acid are given as 5.40×10-7…

Q: What is the pH of a 0.320 M solution of Ca(NO,), (Ka of HNO, is 4.5 × 104)?

A: For HNO2 , pKa = -logKa                           = -log (4.5 x 10-4 )                           =…

Q: Explain the chemical properties of acidic solutions and alkaline solutions taking into consideration…

A: Acids are sour in taste. Acids react with carbonates and hydrogen carbonates to form a salt, water,…

Q: How many grams of dipotassium phtalate (MW = 242.31 g/mol) should be added to 30.00 mL of 0.400 M…

A: Given: Molecular weight of dipotassium phthalate = 242.31 g/mol Volume of HClO4 = 30.00 mL Molarity…

Q: Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively…

A: given, pH of solution = 10.08

Q: The pH of a 0.0031 M solution of HNO, is 3

A:

Q: The compound ethylamine is a weak base like ammonia. A solution contains 0.111 M C,H5NH3* and 0.406…

A:

Q: The pH of a basic solution is 8.41. What is [H1?

A:

Q: Calculate the pH of a 0.299 M NH, solution. NH, has a Kp = 1.8 × 10-5. pH =

A: pH =11.366

Q: 2. An ammonia solution is prepared by diluting 4.00 mL of a 2.00 M solution to 200.0 mL. Give: (a)…

A:

Q: substance with a pH of 2 is?

A:

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

A:

Q: Describe what it means to neutralize (in relation to chemistry and pH)

A:

Q: )A solution made by dissolving 7.40 g of potassium hypochlorite (KClO) into 1.50 L of solution.…

A:

Q: The pH of a 0.0060 M solution of HNO₃ is

A:

Q: 50.0 mL solution is prepared to be 1.29 M acetylsalicylic acid. In the first step, 8.55 mL of NaOH…

A: Volume of solution = 50.0ml  Volume of NaOH = 8.55 ml

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.