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crimeas [40]
3 years ago
8

Changing the number of _____ would change an atom into an atom of a different element

Chemistry
2 answers:
Kamila [148]3 years ago
8 0
Electrons - each atom has its own unique #
Marta_Voda [28]3 years ago
4 0
Changing the number or protons would change the element is an element loses an electron it becomes an ion but if it loses a proton the element its self-changes
eg. calcium has 20 protons if it loses on it becomes potassium that has 19 protons.

Hope that helps :)
You might be interested in
Calculate the change in pH of a 1.00 L of a buffered solution preparing by mixing 0.50 M acetic acid (Ka = 1.8 x 10^-5) and 0.50
tankabanditka [31]

The change in pH of a 1.00 L of a buffered solution preparing by mixing 0.50 M acetic acid (Ka = 1.8 x 10^-5) and 0.50 M sodium acetate when 0.010 mole of NaOH is added is 4.75

when the same amount 0.010 mole of NaOH was added to 1.00 L of water the pH = 12

Explanation:

given that:

concentration of acetic acid = 0.50 M

Concentration of base sodium acetate = 0.50 M

ka = 1.8 x 10^-5)

pka = -log [ka]

pka = 4.74

From Henderson-Hasselbalch Equation:

pH = pKa + log \frac{[base]}{[acid]}

pH = 4.74 + Log \frac{[0.5]}{[0.5]}

pH = 4.74 + 0

pH = 4.74

Number of moles of NaOH = 0.010 moles

volume 1 litre

molarity = 0.010 M

Moles of acetic acid and sodium acetate before addition of NaOH

FORMULA USED:

molarity = \frac{number of moles}{volume in litres}

acetic acid,

0.5 = number of moles

0.5 is the number of moles of sodium acetate.

number of moles of NaOH  0.010 moles

NaOH reacts in 1:1 molar ratio with acetic acid so

number of moles in acetic acid = 0.5 - 0.010 = 0.49

number of moles in sodium acetate = 0.5 +0.010 = 0.51

new pH

pH = pKa + log \frac{[base]}{[acid]}

pH= 4.74 + log[0.51] - log[0.49]

pH= 4.75

PH of NaOH of 0.01 M (BASE)

pOH = -Log[0.01]

pOH         = 2

pH can be calculated as

14= pH +pOH

pH= 14-2

pH = 12

           

8 0
3 years ago
If you want to prepare 5 liters of a 0.35m solution of nh4cl, how many grams of salt
harina [27]
Answer is: mass fo ammonium chloride is 93.625 grams.
V(NH₄Cl) = 5 L.
c(NH₄Cl) = 0.35 M.
n(NH₄Cl) = V(NH₄Cl) · c(NH₄Cl).
n(NH₄Cl) = 5 L · 0.35 mol/L.
n(NH₄Cl) = 1.75 mol.
M(NH₄Cl) = 14 + 1·4 + 35.5 · g/mol = 53.5 g/mol.
m(NH₄Cl) = n(NH₄Cl) · M(NH₄Cl).
m(NH₄Cl) = 1.75 mol · 53.5 g/mol.
m(NH₄Cl) = 93.625 g.
5 0
3 years ago
A hypothesis explains what the scientist thinks will happen during the experiment.
igor_vitrenko [27]

answer: it is true because a hypothesis is something you think will happen during a experiment

explained: I took the test

4 0
3 years ago
When aqueous magnesium chloride reacts with liquid bromine
Bingel [31]
Word equation: magnesium chloride + bromine -> magnesium bromide + chlorine
balance equation: MgCl2 + 2Br -> MgBr2 + 2Cl
3 0
2 years ago
You determine that it takes 26.0 mL of base to neutralize a sample of your unknown acid solution. The pH of the solution was 7.8
Lubov Fominskaja [6]

Complete Question

You determine that it takes 26.0 mL of base to neutralize a sample of your unknown acid solution. The pH of the solution was 7.82 when exactly 13 mL of base had been added, you notice that the concentration of the unknown acid was 0.1 M. What is the pKa of your unknown acid?

Answer:

The pK_a value is pK_a  =7.82

Explanation:

From the question we are told

    The volume of base is  V_B = 26.mL = 0.0260L

     The pH of solution is  pH =  7.82

      The concentration of the acid is C_A = 0.1M

From the pH we can see that the titration is between a strong base and a weak acid

 Let assume that the the volume of acid is  V_A = 18mL= 0.018L

Generally the concentration of base

                    C_B = \frac{C_AV_A}{C_B}

Substituting value  

                     C_B = \frac{0.1 * 0.01800}{0.0260}

                    C_B= 0.0692M

When 13mL of the base is added a buffer is formed

The chemical equation of the reaction is

           HA_{(aq)} + OH^-_{(aq)} --------> A^{+}_{(aq)} + H_2 O_{(l)}

Now before the reaction the number of mole of base is  

            No \ of \ moles[N_B]  =  C_B * V_B

Substituting value  

                    N_B = 0.01300 * 0.0692

                         = 0.0009 \ moles    

                                 

Now before the reaction the number of mole of acid is  

            No \ of \ moles  =  C_B * V_B

Substituting value  

                    N_A = 0.01800 *0.1

                         = 0.001800 \ moles

Now after the reaction the number of moles of  base is  zero  i.e has been used up

    this mathematically represented as

                         N_B ' = N_B - N_B = 0

    The  number of moles of acid is  

             N_A ' = N_A  - N_B

                   = 0.0009\ moles

The pH of this reaction can be mathematically represented as

                 pH  = pK_a + log \frac{[base]}{[acid]}

Substituting values

                  7.82 = pK_a +log \frac{0.0009}{0.0009}

                  pK_a  =7.82        

                     

             

                                 

       

           

                     

8 0
3 years ago
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