Calculate the pH of a solution formed by mixing 100.0 mL of 0.15 M NH4CII with 250.0 ml of 0.20 M NH3. The Kp for NH3 is 1.8 x 10-5. Select one: O 9.78 O 8.73 O 4.22 O 9.35

Q: A 50.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HBr. What is the most likely pH of the…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: Equal quantities of 0.010 M solutions of an acid HA and a base B are mixed. The pH of the resulting…

A: Equilibrium equation : Given data: Equal quantities of 0.010 M solutions of an acid HA and 0.010 M…

Q: A 101.3 mL sample of 0.090 M HCl is mixed with 41.0 mL of 0.090 M NH3.  What is the resulting pH?…

A: Given that

Q: A buffer solution is made that is 0.456 M in HC10 and 0.456 M in KC1O. If Ka for HC10 is 3.50 ×…

A: The Ka for HClO = 3.50×10-8 We have to calculate the pH of a buffer solution that is 0.456 M in HClO…

Q: 17-Consider the following titration curve that corresponds to the titration of a weak acid with a…

A: In the titration of the weak acid and strong base, we get the pKa of the weak acid at the half…

Q: solution made by adding soilid NaClO to water resulted in a baasic equilibrim with a pH of 10.50.…

A: Given data set: Volume = 2 L pH = 10.50 Ka(HClO) = 3.0*10-7 Calculating the value of pOH using the…

Q: The Ką of acid HA is 3.5 x 10 and the Kp of base B is 7.2 x 104. When 0.50-mol HA and 0.50-mol B are…

A: Answer: greater than 7

Q: if 0.030 mole of HCl is added to 0.50 L of the buffer solution (0.24M NH3 and 0.20M NH4Cl) What is…

A:

Q: A buffer solution is made that is 0.450 M in HF and 0.450 M in NaF. If Ka for HF is 7.20 × 10¬4,…

A:

Q: A 75.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the…

A:

Q: A solution contains 0.329 M HA (K₂ = 5.65 · 10−4) and 0.551 M NaA. What is the pH of this solution?…

A:

Q: Suppose you have a buffer, comprised of 0.350 mol of weak base and 0.250 mol of weak acid. Ifthe pH…

A: The of a buffer solution can be calculated using Henderson Hasselbalch Equation written as follows:…

Q: What Is the pH when titrating 27.0 mL of 0.120 M HOCI with 38.0 mL of 0.0900 M NAOH? Ka(HOCI) = 3.0…

A:

Q: A buffer solution is made that is 0.383 M in H₂CO3 and 0.383 M in NaHCO3. If Kal for H₂CO3 is 4.20 x…

A: Given,Molarity of H2CO3 = 0.383 MMolarity of NaHCO3 = 0.383 MKa1 for H2CO3 = 4.20 x 10-7moles of…

Q: 8. 30 mL of 0.100 M HNO3 solution is titrated with a 0.100 M NAOH solution. Find the pH at each of…

A: The question is based on the concept of titrations.   we are titrating  a strong nitric acid with a…

Q: A buffer solution is made that is 0.406 M in HNO2 and 0.406 M in NaNO2. -4 If Ka for HNO2 is 4.50 ×…

A:

Q: What is the pH of a buffer made from 0.350 mol of HBrO and 0.490 mol of KBrO in 2.0 L of solution?…

A:

Q: Consider the titration of a 40.0 mL of 0.115 M weak acid HA (Ka = 2.7 x 10) with 0.100 M LIOH. What…

A:

Q: A buffer is prepared by mixing 16 mL 1M CH3COONa and 4 mL 1M CH3COOH pKa = 4.74. Determine the pH…

A: Buffer capacity of buffer is a measure of magnitude of it`s resistance to change in the pH value on…

Q: A buffer solution is made that is 0.371 M in HCN and 0.371 M in NaCN . (1) If Ka for HCN is…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: A buffer solution is made that is 0.395 M in HCIO and 0.395 M in NaCIO. ces to access important…

A: Given  Concentration of HClO,[HClO] = [Acid] =0.395 M Concentration of NaClO, [NaClO] = [Base] =…

Q: A solution is prepared at 25 °C that is initially 0.27M in chloroacetic acid (HCH₂CICO₂), a weak…

A: pH of buffer solution is calculated by using Henderson Hesselbalch equation.

Q: What is the pH of a buffer solution that is 0.159 M in hypochlorous acid (HCIO) and 0.121 M in…

A: Given: Concentration of hypochlorous acid (HCIO)=0.159 M Concentration of  sodium hypochlorite…

Q: pH

A:

Q: A buffer solution is made that is 0.450 M in HF and 0.450 M in NaF. If Ka for HF is 7.20 × 10-4,…

A:

Q: Consider the titration of a 40.0 mL of 0.153 M weak acid HA (Ka = 2.7 x 10-8) with 0.100 M LİOH.…

A:

Q: CH, NH, is a weak base (Kp = 5.0 x 10-"), so the salt CH, NH, NO, acts as a weak acid. What is the…

A:

Q: potassium hydroxide. (Ka (HBrO) = 2.0 x 10-9) a. What is the initial pH of the solution? HBrO + H₂O…

A: a)when 0.0 mL of KOH is addedHBrO dissociates as:HBrO          ----->     H+   +  BrO-0.8…

Q: A solution was prepared with 0.482 mol of pyridinium fluoride (C, H, NHF) and enough water to make a…

A: Given: Ka= 6.30×10-4 for 0.482M Kb=1.70×10-4 for 1.00L Solution-

Q: )A sample of water containing [Pb2+] = 2.5 × 10−4 M is adjusted to pH 10.80. a)Identify the…

A: The question is based on the concept of solubility product Principle.   it states that a weak…

Q: A buffer is prepared by mixing 0.15 M NazHPO4 and 0.10 M NaH, PO4. K, for H3PO4 = 7.5 103 %3D Ka for…

A: The PH of buffer can be calculated as

Q: The pH at the equivalence point in the titration of 0.10 M HF (k_{a} = 6.3 * 10 ^ - 4) with 0.10 M…

A:

Q: A 75.0 mL sample of 0.100 M NH3 is titrated with 0.100 M HCI. What is the most likely pH of the…

A: Answer :-               pH = 1.845…

Q: You are titrating 30 mL of 0.100M H3PO4 with 0.200 M KOH. For H3PO4: Ka1=1.1X 10-2, Ka2 = 7.5 X…

A: Answer:Moles of any specie in a solution is always equal to the product of its molar concentration…

Q: How many moles of Mg(OH)2 can dissolve in one liter of solution with pH = 10. Ksp Mg(OH)2 = 8.9 x…

A: The expression for the solubility product is given as:Ksp = [Mg2+] [OH-]2 Given: Ksp = 8.9×10-12pH…

Q: Given the following hydrolysis constants, which of the salts has the weakest parent ACID? K₂ or K,…

A: given-hydrolysis constants of given salts.SALTK2 OR K for…

Q: When 40.0 mL of 0.120 M ascorbic acid (C.H: O) is titrated with 0.170 M KOH. Calculate the pH after…

A: The balanced equation for the reaction between  ascorbic acid and KOH is  C6H8O6 (aq)+ KOH (aq)…

Q: A buffer solution is made that is 0.322 M in HCN and 0.322 M in NaCN. (1) If K₂ for HCN is…

A:

Q: What is the pH of a buffer solution that consists of 0.65 M HBrO and 0.38 M KBrO? Ka(HBrO) = 2.3 ×…

A: [acid]=[HBrO]=0.65M [conjugate base]=[kBrO]=0.38M Ka=2.3x10-9 pH=?

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.