A solution is prepared by dissolving 1.50 g of NaOH in enough water to make 1.250 L of solution.  What is the [H3O+] in M of this solution? molar mass of NaOH = 40.0 g/mol

Q: A 0.100 g of Sodium acetate was dissolved in 50 mL D.I water and titrated with 0.055 M HCl.…

A: Mass of sodium acetate dissolved = 0.100 g Volume of sodium acetate solution = 50 mL Molarity of HCl…

Q: What is the approximate value of the equilibrium concentration of A- for the mixture of 0.1 M HCI…

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Q: What is the pH of a 50 cm3 buffer solution if it is contains 0.0100 mol/dm3 sodium acetate and…

A: Acids are categorized as strong acids and weak acids based on the degree of dissociation it…

Q: A buffer solution is prepared in which the concentration of NH3 is 0.20 M and the concentration of…

A: Given : buffer solution of weak acid NH4+ and its conjugate base NH3  concentration of NH3 = 0.20 M…

Q: A buffer solution is made that is 0.431 M in HClO and 0.431 M in NaClO . (1) If Ka for HClO is…

A: pH of the buffer solution is determined by Henderson equation,…

Q: 5 i)What is the pH of a mixture made by adding 0.10 mol of acetic acid and 0.050 mol of potassium…

A: Concentration of acetic acid = 0.10 mol  Concentration of potassium acetate=  0.050 mol  Volume of…

Q: pka = 1.95 (HClO2) If you have 500 mL of a 0.10 M solution of the acid, what mass of the…

A: pH of buffer solution is calculated by using Henderson Hassel balch equation

Q: 0.178 L of aqueous HCl solution of unknown concentration was titrated with 0.825 M KOH (aq). 68.4 mL…

A: here the question:- one unknown M we have to calculate using the ' MVHCl=MVKOH volume of HCl =0.178L…

Q: 2. The weak acid hypochlorous acid (HClO) is formed in bleach solutions. If the pH of a 0.12 M…

A: In multiplart questions we solve only three subquestion according to Bartleby Guidelines. pH of any…

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: >Calculate pH of a solution of a 0.10 M CH3COOH solution? Ka = 1.8 X 10-5 How many grams of CH3COOh…

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Q: A buffer solution is prepared by dissolving 0.200 mol of NaH 2PO 4 and 0.100 mol of NaOH in enough…

A: Buffer solution is the solution which has tendency to maintain constant pH upon addition of small…

Q: Calculate the weights of Mg(OH)2 that will dissolve in  a) 250 mL of water b) 250 mL of a buffer…

A: Step-1 Let the solubility of Mg(OH)2 in 250 mL of water be ‘s’ Ksp = [S][2S]2 Ksp = 4S3 5.6 x 10-12…

Q: A 25.00 mL sample of methanoic (HCHO2, Ka = 1.8 x 10-4) is titrated to the equivalence point using…

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Q: A buffer solution is made that is 0.440 M in HClO and 0.440 M in NaClO. (1) If Ka for HClO is…

A: Given : Concentration of weak acid HClO = 0.440 M And concentration of conjugate base salt of weak…

Q: The concentration of Mg 2+ in seawater is 0.052 M. At what pH will 99% of the Mg 2+ be precipitated…

A: We have 0.052 M of Mg+2 , we have to predict the pH at which 99% of Mg+2 will be precipitated .

Q: Calculate the pH of a buffer that is 0.130 M in NaHCO3 and 0.335 M in Na2CO3.

A: pH is used to determine the concentration of hydronium ion.

Q: Calculate the pH of the buffer that results from mixing 53.1 mL of a 0.322 M solution of HCHO2 and…

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Q: Calculate the pH of 0.45 M solution of methylamine, CH3NH2 , and 0.25 M methylammonium bromide…

A: Basic solutions containing salt ions and weak base perform special function of maintaining constant…

Q: What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.240 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 ×…

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Q: What is the pH of a buffer solution that contains 0.25 M HClO and 0.35 M NaClO? (pKa HClO = 7.46)…

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Q: _______6. Na2 CO3   forms alkaline solution when dissolved in water. Why? Because water hydrolysis…

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Q: 6. Compute for the pH, pOH, and [OH-] of a buffer solution that is 0.30 M in acetic acid and…

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Q: How many grams of sodium acetate (82.03 g/mol) must be added to 1.00 L of 0.50 M solution of acetic…

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Q: could you please answer and show working to the following questions    1. What is the pH of a…

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Q: 47. What is the pH of the buffer that results when 4.2 g of NH; (MW = 17.03 g/mol) and 4.6 g of…

A: The pH can be calculated as follows

Q: Typical "hard" water contains about 80.2 mg of Ca2* per liter. Calculate the maximum concentration…

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Q: 00 mL of a buffer solution contains 0.050 mol NaHSO3 and 0.031 mol Na2SO3. (pKa = 7.172). What is…

A: By the Henderson- Hasselbalch equation, pH = pKa + log [salt]/[acid]

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: What is the pH of a buffer solution of 0.0025 M CH 3CO 2H and 0.00125 M CH 3CO 2Na? ( K a = 1.8 × 10…

A: Henderson-Hasselbalch equation Henderson-Hasselbalch equation explains the relationship between pH…

Q: a. What quantity (moles) of NaOH must be added to 1.0 L of 1.7 M HC, H3O2 to produce a solution…

A: Here we have to determine the moles of NaOH should be added to 1Liter of 1.7 M CH3COOH to make the…

Q: Consider a buffer solution that is 0.50 M in NH and 0.20 M in NH4Cl. For ammonia, pKp = 4.75.…

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Q: Why are Ce4+solutions never used for the titration of reductants in basic solutions?

A: The reason why Ce4+ solutions are not used for the titration of reductants in basic solutions have…

Q: From the value of Kf, calculate the concentration of Ni2+ (aq) and Ni(NH3)62+ that are present at…

A: Given: Mass of NiCl2=1.25 g Volume of NH3(aq)=100 mL Concentration of NH3(aq)=0.20 M

Q: Calculate the pH of a 0.654 M solution of an acid with Ka = 2.33 x 10-5.

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Q: What is the solubility of magnesium hydroxide in a solution buffered at pH 8.95? K„ (Mg(OH)2) = 1.8…

A: Concentration of OH- can be calculated as follows:

Q: A buffer solution is prepared by dissolving 27.22g of KH2PO4 and 3.37g of KOH in enough water to…

A: KH2PO4 + KOH = K2HPO4 + H2O  So, KH2PO4 and K2HPO4 acts as acid and salt made from strong base with…

Q: CH3COOH

A: A) mmoles of Acid = 25mL • 0.2molL-1 = 5.0mmol  B) mmoles of Base = 35mL • 0.1molL-1 = 3.5mmol…

Q: One strategy for dealing with the acidification of lakes is periodically to add powered limestone…

A: Solution - According to the question - Given -  Ksp expression for CaCO3 is Ksp = [Ca2+] [CO32-]…

Q: what is the pH at the equivalent point in the titrafion of 5 mmol Potassium acid phthalate dissolved…

A: Solution :        The solution which resists any change in pH on the addition of a small amount of…

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

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Q: 1. Calculate the [H+] and the pH of a buffer solution that is 0.10 M in CH3COOH (Ka = 1.8 x 10-5)…

A: The  concentration of H+ and the pH of a buffer solution are calculated in step two.

Q: 1. A 0.0250 M Ca(X)₂ has a pH of 8.049. Ca(X)₂ is composed of a Ca²+ cation and an unknown anion X,…

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

Q: the PH of the acid before any base solution is added

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Q: Phosphoric acid is a triprotic acid (?a1=6.9×10^3Ka1=6.9×10^3, ?a2=6.2×10^8 Ka2=6.2×10−8, and…

A: Buffer solutions are those solutions which resist the change in pH upon addition of small amount of…

Q: Consider a buffer solution prepared by adding 0.45 mol of CH3COOK to 1.00 L of 2.00 M CH3COOH. (K₁ =…

A: The given buffer solution is an acidic buffer solution which is made up of weak acid (CH3COOH) and…

Q: What is the pH of a buffer solution that contains 0.25 M HClO and 0.35 M NaClO? (pKa HClO = 7.46)…

A: Given  PKa  = 7.46 Concentration of HClO acid   =  0.25 M  Concentration of NaClO salt  =  0.35 M…