What is the pH of a solution of 0.400 M CH3NH2 containing 0.210 M CH;NH31? (Kb of CH;NH2 is 4.4 × 10-4)

Q: What mass of NaCN must be added to 1 L of 0.010 M Mg(NO3)2 in order to produce the first trace of…

A: Given:

Q: Calculate the pH of a 0.23 M sodium formate solution (HCOONA). Kp for HCOO = 5.9 x 10-11

A: Given that,    Concentration of HCOONa solution = 0.23 M   Kb for HCOO-  = 5.9×10-11  Since, pKb =…

Q: What is the pH of 3 22e-3 M HCIO3?

A:

Q: What is the pH of a 0.70M KCN solution at 25oC (HCN, Ka=6.17*10-10)

A: Given: 0.70 M KCN solution. Ka of HCN is 6.17*10-10

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.200 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: By using Henderson Hasselbalch equation the pH of the buffer solution is determined by using the…

Q: What is the pH of a 0.260 M solution of aniline (C6HSNH2, Kb = 4.3 x 10-10)?

A: Given, MOlarity of aniline = 0.260M

Q: What is the pH of a 0.150 M solution of aniline (CeH;NH2, Kb = 4.3 × 10-1º)?

A:

Q: What is the pH of a 0.310 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)

A: Since aniline is a weak base. Hence it will dissociate as  C₆H₅NH₂ (aq) + H2O (l) ------->…

Q: What is the pH of a 0.290 M solution of aniline (C6H5NH2, Kb = 4.3 x 10-10)?

A: In the given question we have to calculate the pH of Aniline. concentration of Aniline = 0.290 M  Kb…

Q: calculate the ph of a .36 M of ethylamine and .52 M methylammonium bromide CH3CH2NH3Br. the base…

A: Basic buffer solution consists of a weak base and its conjugate salt. ethylamine is the weak base…

Q: 3. Determine the pH of aqueous of 0.100 M solutions of the following salts. The provided K₂ and Kb…

A: The answer to the following question is-

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.110 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A:

Q: magnesium hydroxide has Ksp = 5.61 × 10-¹². a) What will be the pH when we add 1 mol of MgCl2 to a…

A: Ksp represent solubility product and it gives an idea about the product of ion during saturated…

Q: What is the pH of 1.10 M CrCl3 (K = 1.00x10-4)? %3D

A: Given, Concentration of CrCl3 (C) = 1.10 M Ka = 1.00 × 10-4 pH of the solution = ? Note: pKw = 14…

Q: What is the pH of a 0.03 M solution of sodium benzoate (C6H5COONa)? Ka = 6.6 *10-5.

A: It is given that 0.03 M sodium benzoate (C6H5COONa) is present, and the equation is written as…

Q: Calculate the pH of a 0.450 M solution of NH4Cl (Kb for NH3 is 1.8 x 10-5)

A: Interpretation -  To determine the pH of 0.45M of NH4Cl solution when Kb of NH3 = 1.8 ×10-5 .…

Q: What is the pH of a 0.0125 M hyploclorous acid? (Ka= 3.0 x 10-8)

A:

Q: What is the pH of a 0.870 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)? 1 4 6. 3. LO

A: Data given Ka = 4.5 x10^-4  Concentration of Ca(No2)2 = 0.870 M

Q: calculate the pH of a solution that is 1.00 M CH3COOH (ka = 1.0 x 10^-5) and 1.00 M CH3COONa

A: Given: Concentration of weak acid CH3COOH = 1.00 M And the concentration of CH3COONa = 1.00 M

Q: What is the pH of a 0.36 M solution of HNO2 (Ka = 4.5 x 10-4)?

A:

Q: A sample of water at pH 10.5 has 75 mg/L of CO3-2 and 65 mg/L of HCO3- Including the contribution of…

A:

Q: 5- Calculate the formal concentration of 12% (w/w) CUSO4 solution which has density of 1.13 g/mL.

A: Formal concentration is the number of moles of formula units present per litre of solution.  Given:…

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. At 25°C, what are the molar H,O* and OH concentrations in a. 0.0300 M C6H5COOH? b. o.обоо М HN3?…

A: Interpretation -  To determine the concentration of H3O+  and OH- in the -  0.03M C6H5COOH   0.06M…

Q: The Ka of CH3COOH is 1.8 x 10-5. Calculate the pH of a solution containing both 0.20 M CH3COOH and…

A:

Q: 6-39. An acidic solution containing 0.010 M La 3+ is treated with NaOH until La(OH), precipitates.…

A: Given information, Concentration of La3+ = 0.010 M Reaction : La3+ (aq) + NaOH (aq) --> La(OH)3…

Q: Calculate the pH of 0.1 M from sodium acetate CH3CO2Na and hydrolysis percent ? if you know Ka =…

A: Reaction of sodium acetate in water can be written as, CH3COONa + H2O →CH3COOH +Na+ + OH-

Q: What is the pH of a 0.650 M solution of C5H;NHB (Kb of CsH;N is 1.7 × 10-º)?

A:

Q: What is the pH of a solution containing 0.30 M lactic acid (K₂ = 1.38 x 10-4) and 0.50 M of lactate…

A:

Q: What is the pH of a 0.280 M solution of aniline (C6H;NH2, Kb = 4.3 × 10-1º)? %3D

A:

Q: Calculate the pH of 3.5M citric acid solution at 25⁰C when the Ka is 7.1 x 10-4.

A: Give information: Concentration of solution = 3.5 M Ka is 7.1 x 10-4

Q: 5.) What is K, for an acid whose pk, is 3.78?

A: This is the concept of converting terms

Q: A solution of H2PO-4 had a [H3O+] of 2.9e-2 M. What was the pH?

A: pH = - log[H3O+]

Q: What is the pH of a 0.660 M solution of C3H;NHB (Kb of C5H5N is 1.7 x 10-9)?

A: Given information, [C5H5NHBr] = 0.660 M Kb of C5H5N = 1.7*10-9 Calculate: pH = ?

Q: Explain why-(i) Anhydrous calcium chloride is used in desiccators(ii) If bottle full of concentrated…

A: i) Anhydrous calcium chloride CaCl2 is highly hygroscopic in nature it readily absorbs moisture.…

Q: What is the pH of a solution of 0.300 M HNO2 containing 0.120 M NaNO2? (Ka of HNO2 is 4.5 × 10¬4)

A: The given data contains, Concentration of weak acid =0.300M Concentration of conjugate base =0.120M…

Q: What are the concentrations of H3O+ and OH− in oranges that have a pH of 3.97?

A:

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.150 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: In this question, we will calculate the pH of this solution ( this is a buffer solution ). For…

Q: 10-13. How many milliliters of 0.202 M NaOH should be added to 25.0 mL of 0.023 3 M salicylic acid…

A: We know that  pH of buffer is  pH = pka + log {[salt] / [ acid]}

Q: What is the pH of a 0.64 M solution of NH3 (Kb = 1.2 × 10-5)?

A:

Q: Consider a weak acid, HA, for which Ka = 7.1x10-4. Calculate [H*] in a solution that is 0.45 M in…

A:

Q: What is the mole ratio of sodium acetate to acetic acid in abuffer with a pH of 5.75?

A:

Q: What is the pH of the ethanoic acid solution CH3COOH 0.15 M with Ka = 1.8 × 10-⁵? b) What will be…

A: Molar mass of sodium ethanoate= 82 g/mol nsodium ethanoate = 82g / (82 g/mol) = 1 mol Ka = 1.8 X…

Q: what is the pH of a 50 mg mL-1 solution of ascorbic acid (MW 176.1, pKa 4.17)?

A: Ascorbic acid dissociates in water as: C6H8O6+H2O→C6H7O6-+H+ -------(1)

Q: What is the pH of a solution of 0.400 M CH;NH2 containing 0.140 M CH;NH31? (Kb of CH;NH2 is 4.4 ×…

A:

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.210 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: BUFFER SOLUTION It is a solution of weak acid or base with their corresponding conjugate base or…

Q: What is the pH of a 0.0245 M solution of NH3?        Kb = 1.8 x 10-5

A:

Q: The acid ionization constant for Sc(H2O)63+ (aq) is 5.0×10-5 . Calculate the pH of a 0.0043 M…

A: Given , acid ionisation constant , Ka= 5.0×10-5 concentration of the Sc(NO3)3= 0.0043 M

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

A: Using the equilibrium concept  We can calculate the H+ concentration

Q: What is the pH of a 1.20 M nitrous acid solution? (Ka = 4.50 x 10-4)

A:

Matter and Measurement

In the universe, there is matter, energy, and void space. The universe contains energy and void space. The definition of matter can be considered as something which possesses mass and consumes space. Chemistry is that branch of science which deals with the study of matter. Under chemistry, nature, composition, and the changes occurring to matter are discussed.